2 KNO3 (aq) + PbCl2 (s)}\]. Aqueous nickel(II) nitrate + aqueous sodium hydroxide, 8. The balanced equation will appear above. # $ % & ' �������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������� ` �� � bjbj�� c �� �� 5_ x �� �� �� � � � � � � � � � T � � � @ \� � �� \ T � l H� H� : �� �� �� �� �� �� � � � � � � � $ h o � A � A� �� �� A� A� � � �� �� U /� /� /� A� | � �� � �� � /� A� � /� /� � �� � � � b� ��. Since one of the predicted products is insoluble, a precipitation reaction is will occur. Hydrochloric acid + aqueous sodium hydroxide, 10. Some of the observable signs that a chemical reaction has occurred include the following: Note that there are many other observable signs for chemical reactions, but these are the ones most likely to be encountered in this lab. Product Names & States (if none, why not? However sulfurous acid decomposes to sulfur dioxide and water: \[\ce{2 HNO3 (aq) + Na2SO3 (aq) -> 2 NaNO3 (aq) + H2SO3 (aq)} \text{(decomposes)}\], \[\ce{2 HNO3 (aq) + Na2SO3 (aq) -> 2 NaNO3 (aq) + H2O (l) + SO2 (g)}\], Solids: Copper metal, zinc metal, magnesium metal, solid sodium bicarbonate. A student titrates an unknown concentration of NaOH solution with H2SO4 according to the following balanced equation. Here \(AB\) and \(CD\) are usually aqueous ionic compounds (or acids) consisting of aqueous ions (\(A^+\) and \(B^-\), \(C^+\) and \(D^-\)). Aqueous sodium phosphate + aqueous copper(II) sulfate, 5. To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. If the word equation is complete, write and balance the chemical equation. As a rule, if A has a higher activity that \(B\), a single displacement reaction will occur. If no reaction occurs write the words "no reaction" (or NR) instead of the products in your balanced equation and indicate why your think there was no reaction. Write the correct formulas for each reactant and place a yield arrow (→) after the last reactant. Use approximately 3-mL quantities of all solutions. Balanced Molecular Equation (from page 1): Balanced Molecular Equation (from page 3): Predict the products for the following single and double displacement reactions, and write balanced molecular equations (including physical states) for each of them. Neutralization reactions are exothermic, and are generally accompanied by a noticeable release of heat. To balance it, we must place the coefficient 5 on the left of oxygen on the left side of the equation to balance the oxygen atoms appearing on the right side of the equation. Aluminum metal + aqueous nickel(II) nitrate. To become familiar with some of the observable signs of these reactions. The predicted products are aluminum metal and aqueous magnesium chloride, \[\ce{3 Mg (s) + 2 AlCl3 (aq) -> 2 Al (s) + 3 MgCl2 (aq)}\]. THE IDEAL-GAS EQUATION 391 Relating the Ideal-Gas Equation and the Gas Laws 394 10.5 FURTHER APPLICATIONS OF THE IDEAL-GAS EQUATION 395 Gas Densities and Molar Mass 396 Chemical Reactions 397 10.6 Volumes of Gases in GAS MIXTURES AND PARTIAL PRESSURES 399 Partial Pressures and Mole Fractions 400 Water 401 10.7 Collecting Gases over Perform the following reactions and record your observations for each on the report form. Tell the type of reaction. A precipitate (cloudy, tiny particles) appears. b. is the reactant for which you have the fewest number of moles. Be sure to include the physical states of all reactants and products in your final equation. The balanced equation for the reaction is 3O2 1g2 ¡ 2O3 1g2 To calculate the moles of O3 produced, we must use the appropriate mole ratio: 0.50 mol O2 lh h C b di b k i h h i d i i 2 mol O3 0.33 mol O3 3 mol O2 Avogadro’s law states that V an, which can be rearranged to give N2 H2 An excess of NaOH … Note that some reactions take longer than others. Always use clean test tubes that have been rinsed with distilled water. Solid sodium bicarbonate + acetic acid, 6. The test tubes do not have to be dry. \[\ce{H2SO4 (aq) + 2 LiOH (aq) -> Li2SO4 (aq) + 2 H2O (l)}\]. The balanced equation will appear above. This solid product is an insoluble ionic compound called a precipitate. Analytical Chemistry Douglas A. Skoog, Donald M. West, F. James Holler, Stanley R. Crouch If the new element \(B\)is a metal, it will appear as a metallic deposit. The balanced equation describes the stoichiometry (b) The scale of the reaction is determined by the number of moles used as reactants in the experiment. To write balanced chemical equations for each single and double displacement reaction studied. predict the reaction type (single or double displacement), write the balanced “molecular” equation, including all, Consider Reactions 3 and 14 studied in this lab. All waste is to be disposed of in the plastic container in the hood! Equipment: 6 large test tubes, 8 small test tubes, plastic test tube rack (or large beaker). Write the balanced molecular equation (identical to what you completed in the previous section), the complete ionic equation and the net ionic equation for these reactions. What is the general equation of a single displacement reaction? ��ࡱ� > �� ( * ���� ! " If you determine that a reaction will not occur, simply write “no reaction” after the arrow. The ash was dissolved in 60meq HCl and the resulting solution was back titrated with NaOH. Alkali metal compounds, acetates, nitrates, and ammonium compounds are all, Hydroxides of alkali metals and \(\ce{NH4^{+1}}\), \(\ce{Ca^{+2}}\), \(\ce{Sr^{+2}}\), and \(\ce{Ba^{+2}}\) are, Most phosphates, carbonates, chromates and sulfides are, Aqueous barium chloride + aqueous sodium sulfate, Aqueous sodium phosphate + aqueous copper(II) sulfate, Aqueous nickel(II) nitrate + aqueous sodium hydroxide, Aqueous potassium chloride + aqueous silver nitrate, Hydrochloric acid + aqueous sodium hydroxide, Aqueous sodium carbonate + aqueous cobalt(II) nitrate, Aqueous sodium chloride + aqueous potassium nitrate, Aqueous iron(III) chloride + aqueous ammonium hydroxide. Aqueous zinc chloride + aqueous sodium chromate, Aqueous lithium hydroxide + phosphoric acid. However, if \(A\) has lower activity than \(B\), a single displacement reaction will not occur. Solutions: 6 M sodium hydroxide, 6 M hydrochloric acid, 6 M ammonium hydroxide, 5% acetic acid; all other solutions are 0.1 M and include silver nitrate, barium chloride, sodium sulfate, potassium chloride, lead(II) nitrate, iron(III) chloride, sodium carbonate, cobalt(II) nitrate, sodium phosphate, zinc nitrate, copper(II) sulfate, sodium chloride, potassium nitrate, nickel(II) nitrate. To determine whether a product ionic compound will be soluble or insoluble, consult the Solubility Rules provided at the end of the Background section. 1. magnesium metal + aqueous aluminum chloride, Since \(\ce{Mg}\) is more active than \(\ce{Al}\), a single displacement reaction will occur. What is the general equation of a double displacement reaction? Aqueous iron(III) chloride + aqueous ammonium hydroxide, Reaction 3: Aqueous sodium phosphate + aqueous copper(II) sulfate, Reaction 14: Aqueous iron(III) chloride + aqueous ammonium hydroxide. Adopted a LibreTexts for your class? If the word equation is incomplete, complete it and write the balanced chemical equation. If Avogadro number N A , is changed from 6.022 × 1023 mol 1 to 6.022 × 10 20 mol 1, this would change (a) the mass of one mole of carbon (b) the ratio of chemical species to each other in a balanced equation (c) the ratio of elements to each other in a compound (d) the definition of mass in units of grams. Then write a balanced equation for each reaction. An Activity Series is provided at the end of the Background section. Use uppercase for the first character in the element and lowercase for the second character. Examples: Fe, Au, Co, Br, C, O, N, F. Ionic charges are not yet supported and will be ignored. For the reactions involving solid reactants (#2, 4, 5, 7, 11, 13), use the large test tubes. Aqueous zinc nitrate + aqueous lithium chloride, Hydrobromic acid + solid magnesium sulfite, Aqueous rubidium hydroxide + perchloric acid, Aqueous lithium chromate + aqueous gold(III) iodide. Consider Reactions 3 and 14 studied in this lab. Old substances are converted to new substances, which have unique physical and chemical properties of their own. C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) 51 Determine the mass of CO2 produced when 9.0 grams of glucose completely reacts with 9.6 grams of oxygen to produce 5.4 grams of water. Here \(AB\) is an acid (consisting of \(H^+\) and \(X^-\) aqueous ions) and \(BC\) is a base (consisting of \(M^+\) and \(OH^-\) ions). Identify the reaction type – single or double displacement, using the guidelines outlined thus far. aqueous lead(II) nitrate + aqueous potassium chloride. However, one of the products could also be carbonic acid (\(\ce{H2CO3}\)) or sulfurous acid (\(\ce{H2SO3}\)). The limiting reactant in a reaction: a. has the lowest coefficient in a balanced equation. Click here to let us know! If you determine that a reaction will occur, write the correct formula(s) of the products after the arrow. 12 meq of NaOH were required to reach end point. Ported Sub Box Meaning, Manoj Bharathiraja Movies, Santa Clara County Property Records, Halo 2 Scarab Skull, Brett Brown Wife Picture, Cuando Empieza El Celo De Una Gata, " />

h2so3 and naoh balanced equation

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To identify the products formed in each of these reactions. Balance the equation (to ensure mass conservation). Academia.edu is a platform for academics to share research papers. The balanced equation below represents the reaction of glucose, C6H12O6, with oxygen at 298 K and 101.3 kPa. 4.25. Be sure to include the states of all compounds in your equations (solid, liquid, aqueous, or gas). If you determine that a reaction will not occur, write “NR”, and provide a brief explanation. Examples: Fe, Au, Co, Br, C, O, N, F. Ionic charges are not yet supported and will be ignored. Give reason(s) for the product(s) 1. barium chloride + sodium sulfate → 2. calcium + hydrochloric acid → 3. ): 3. In the reactions involving both a solid and a solution as reactants, which do you place in the test tube first? Aqueous sodium carbonate + cobalt(II) nitrate, 11. The equipment required for this lab is fairly simple - just 8 small test tubes and 6 large test tubes. Thus, if results are not obtained immediately, give the reaction some time. To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. 5.0 Approximately what mass of CuSO4•5H2O (250 g mol-1) is required to prepare 250 mL of 0.10 M copper(II) sulfate solution? To perform and observe the results of a variety of single and double displacement reactions. Use uppercase for the first character in the element and lowercase for the second character. Place the metal in the test tube first, and then add the solution. NH4+ is the conjugate acid to the base NH3, because NH3 gained a hydrogen ion to form NH4+.The conjugate base of an acid is formed when the acid donates a proton. Inform your instructor of any chemical contact as soon as possible. For each of the following sets of reactants, write the balanced equation for the double displacement reaction that occurs. 4.24. All single displacement reactions have the general form: Here, \(A\) is an element and \(BC\) is usually an aqueous ionic compound or an acid (consisting of \(B^+\) and \(C^-\) aqueous ions). If you predict that no reaction will occur, write “NR”, followed by a brief explanation. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Zinc metal + aqueous lead(II) nitrate, 12. In these reactions one of the products (\(AD\) or \(CB\)) after the double displacement is in the gaseous state. A good estimate is to use two full dropper squirts of each chemical. Note that if both of the predicted products are soluble, a precipitation reaction will not occur. The LibreTexts libraries are Powered by MindTouch® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. In this lab you will perform a variety of single and double displacement reactions. The metal should be completely immersed in the solution used. Conjugate acids and conjugate bases are the acids and bases that lose or gain protons. All double displacement reactions have the general form: Reactions that can be classified as double displacements include precipitation reactions, neutralization reactions and gas forming reactions. If you determine that a reaction will not occur, write “NR”, and provide a brief explanation. sulfuric acid + aqueous lithium hydroxide. Aqueous barium chloride + aqueous sodium sulfate. Legal. If it is a gas, it will appear as bubbles. Be especially cautious when using the 6 M \(\ce{HCl}\) and 6 M \(\ce{NaOH}\) as they can burn your skin. The predicted products are water and lithium sulfate. Aqueous sodium chloride + aqueous potassium nitrate, 14. When finished, complete your lab report by writing the balanced equations for each reaction studied. Include all. Unless otherwise noted, LibreTexts content is licensed by CC BY-NC-SA 3.0. What are three observable signs that a chemical reaction has occurred? The predicted products are lead(II) chloride (insoluble) and potassium nitrate (soluble). Aqueous potassium chloride + aqueous silver nitrate, 9. According to the balanced equation above, how many moles of HI would be necessary to produce 2.5 mol of I2, starting with 4.0 mol of KMnO4 and 3.0 mol of H2SO4 ? During a chemical reaction both the form and composition of matter are changed. 2H2O2 2H2O + O2. One such example is hydrogen sulfide (\(\ce{H2S}\)). Write the balanced molecular equation (identical to what you completed in the previous section), the complete ionic equation and the net ionic equation for these reactions. Include all physical states, and circle the spectator ions in the complete ionic equations. For reactions involving solutions only, use small test tubes. 6: Single and Double Displacement Reactions (Experiment), [ "article:topic", "authorname:smu", "showtoc:no", "license:ccbync" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FAncillary_Materials%2FLaboratory_Experiments%2FWet_Lab_Experiments%2FGeneral_Chemistry_Labs%2FOnline_Chemistry_Lab_Manual%2FChem_10_Experiments%2F06%253A_Single_and_Double_Displacement_Reactions_(Experiment), 5: The Composition of Potassium Chlorate (Experiment), 7: Mole Ratios and Reaction Stoichiometry (Experiment), Pre-laboratory Assignment: Single and Double Displacement Reactions, Lab Report: Single and Double Displacement Reactions, information contact us at info@libretexts.org, status page at https://status.libretexts.org. Have questions or comments? For each of the following sets of reactants, write the balanced equation for the single displacement reaction that occurs. If you feel any tingling sensations or see any color changes on your skin, flush with water immediately for a minimum of 15 minutes. When a double displacement reaction occurs, the cations and anions switch partners, resulting in the formation of water and a new ionic compound (or salt), which is usually soluble. An Activity Series of elements is often used to determine if \(A\) will displace \(B\) in a single displacement reaction. A displaces \(B\) in \(BC\), resulting in the formation of a new element \(B\) and a new ionic compound or acid, \(AC\). For more information contact us at info@libretexts.org or check out our status page at https://status.libretexts.org. When a double displacement reaction occurs, the cations and anions switch partners, resulting in the formation of two new ionic compounds AD and CB, one of which is in the solid state. (2015) (a) 8 : 16 : 1 (c) 16 : 1 : 2 Also be aware that skin discoloration will result from contact with \(\ce{AgNO3}\). Both carbonic acid and sulfurous acid are unstable and will decompose to form carbon dioxide and sulfur dioxide gases, respectively: The predicted products are sulfurous acid and sodium nitrate. For reactions involving metals, use just 1-2 pieces of each metal. \[\ce{Pb(NO3)2 (aq) + 2 KCl (aq) -> 2 KNO3 (aq) + PbCl2 (s)}\]. Aqueous nickel(II) nitrate + aqueous sodium hydroxide, 8. The balanced equation will appear above. # $ % & ' �������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������� ` �� � bjbj�� c �� �� 5_ x �� �� �� � � � � � � � � � T � � � @ \� � �� \ T � l H� H� : �� �� �� �� �� �� � � � � � � � $ h o � A � A� �� �� A� A� � � �� �� U /� /� /� A� | � �� � �� � /� A� � /� /� � �� � � � b� ��. Since one of the predicted products is insoluble, a precipitation reaction is will occur. Hydrochloric acid + aqueous sodium hydroxide, 10. Some of the observable signs that a chemical reaction has occurred include the following: Note that there are many other observable signs for chemical reactions, but these are the ones most likely to be encountered in this lab. Product Names & States (if none, why not? However sulfurous acid decomposes to sulfur dioxide and water: \[\ce{2 HNO3 (aq) + Na2SO3 (aq) -> 2 NaNO3 (aq) + H2SO3 (aq)} \text{(decomposes)}\], \[\ce{2 HNO3 (aq) + Na2SO3 (aq) -> 2 NaNO3 (aq) + H2O (l) + SO2 (g)}\], Solids: Copper metal, zinc metal, magnesium metal, solid sodium bicarbonate. A student titrates an unknown concentration of NaOH solution with H2SO4 according to the following balanced equation. Here \(AB\) and \(CD\) are usually aqueous ionic compounds (or acids) consisting of aqueous ions (\(A^+\) and \(B^-\), \(C^+\) and \(D^-\)). Aqueous sodium phosphate + aqueous copper(II) sulfate, 5. To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. If the word equation is complete, write and balance the chemical equation. As a rule, if A has a higher activity that \(B\), a single displacement reaction will occur. If no reaction occurs write the words "no reaction" (or NR) instead of the products in your balanced equation and indicate why your think there was no reaction. Write the correct formulas for each reactant and place a yield arrow (→) after the last reactant. Use approximately 3-mL quantities of all solutions. Balanced Molecular Equation (from page 1): Balanced Molecular Equation (from page 3): Predict the products for the following single and double displacement reactions, and write balanced molecular equations (including physical states) for each of them. Neutralization reactions are exothermic, and are generally accompanied by a noticeable release of heat. To balance it, we must place the coefficient 5 on the left of oxygen on the left side of the equation to balance the oxygen atoms appearing on the right side of the equation. Aluminum metal + aqueous nickel(II) nitrate. To become familiar with some of the observable signs of these reactions. The predicted products are aluminum metal and aqueous magnesium chloride, \[\ce{3 Mg (s) + 2 AlCl3 (aq) -> 2 Al (s) + 3 MgCl2 (aq)}\]. THE IDEAL-GAS EQUATION 391 Relating the Ideal-Gas Equation and the Gas Laws 394 10.5 FURTHER APPLICATIONS OF THE IDEAL-GAS EQUATION 395 Gas Densities and Molar Mass 396 Chemical Reactions 397 10.6 Volumes of Gases in GAS MIXTURES AND PARTIAL PRESSURES 399 Partial Pressures and Mole Fractions 400 Water 401 10.7 Collecting Gases over Perform the following reactions and record your observations for each on the report form. Tell the type of reaction. A precipitate (cloudy, tiny particles) appears. b. is the reactant for which you have the fewest number of moles. Be sure to include the physical states of all reactants and products in your final equation. The balanced equation for the reaction is 3O2 1g2 ¡ 2O3 1g2 To calculate the moles of O3 produced, we must use the appropriate mole ratio: 0.50 mol O2 lh h C b di b k i h h i d i i 2 mol O3 0.33 mol O3 3 mol O2 Avogadro’s law states that V an, which can be rearranged to give N2 H2 An excess of NaOH … Note that some reactions take longer than others. Always use clean test tubes that have been rinsed with distilled water. Solid sodium bicarbonate + acetic acid, 6. The test tubes do not have to be dry. \[\ce{H2SO4 (aq) + 2 LiOH (aq) -> Li2SO4 (aq) + 2 H2O (l)}\]. The balanced equation will appear above. This solid product is an insoluble ionic compound called a precipitate. Analytical Chemistry Douglas A. Skoog, Donald M. West, F. James Holler, Stanley R. Crouch If the new element \(B\)is a metal, it will appear as a metallic deposit. The balanced equation describes the stoichiometry (b) The scale of the reaction is determined by the number of moles used as reactants in the experiment. To write balanced chemical equations for each single and double displacement reaction studied. predict the reaction type (single or double displacement), write the balanced “molecular” equation, including all, Consider Reactions 3 and 14 studied in this lab. All waste is to be disposed of in the plastic container in the hood! Equipment: 6 large test tubes, 8 small test tubes, plastic test tube rack (or large beaker). Write the balanced molecular equation (identical to what you completed in the previous section), the complete ionic equation and the net ionic equation for these reactions. What is the general equation of a single displacement reaction? ��ࡱ� > �� ( * ���� ! " If you determine that a reaction will not occur, simply write “no reaction” after the arrow. The ash was dissolved in 60meq HCl and the resulting solution was back titrated with NaOH. Alkali metal compounds, acetates, nitrates, and ammonium compounds are all, Hydroxides of alkali metals and \(\ce{NH4^{+1}}\), \(\ce{Ca^{+2}}\), \(\ce{Sr^{+2}}\), and \(\ce{Ba^{+2}}\) are, Most phosphates, carbonates, chromates and sulfides are, Aqueous barium chloride + aqueous sodium sulfate, Aqueous sodium phosphate + aqueous copper(II) sulfate, Aqueous nickel(II) nitrate + aqueous sodium hydroxide, Aqueous potassium chloride + aqueous silver nitrate, Hydrochloric acid + aqueous sodium hydroxide, Aqueous sodium carbonate + aqueous cobalt(II) nitrate, Aqueous sodium chloride + aqueous potassium nitrate, Aqueous iron(III) chloride + aqueous ammonium hydroxide. Aqueous zinc chloride + aqueous sodium chromate, Aqueous lithium hydroxide + phosphoric acid. However, if \(A\) has lower activity than \(B\), a single displacement reaction will not occur. Solutions: 6 M sodium hydroxide, 6 M hydrochloric acid, 6 M ammonium hydroxide, 5% acetic acid; all other solutions are 0.1 M and include silver nitrate, barium chloride, sodium sulfate, potassium chloride, lead(II) nitrate, iron(III) chloride, sodium carbonate, cobalt(II) nitrate, sodium phosphate, zinc nitrate, copper(II) sulfate, sodium chloride, potassium nitrate, nickel(II) nitrate. To determine whether a product ionic compound will be soluble or insoluble, consult the Solubility Rules provided at the end of the Background section. 1. magnesium metal + aqueous aluminum chloride, Since \(\ce{Mg}\) is more active than \(\ce{Al}\), a single displacement reaction will occur. What is the general equation of a double displacement reaction? Aqueous iron(III) chloride + aqueous ammonium hydroxide, Reaction 3: Aqueous sodium phosphate + aqueous copper(II) sulfate, Reaction 14: Aqueous iron(III) chloride + aqueous ammonium hydroxide. Adopted a LibreTexts for your class? If the word equation is incomplete, complete it and write the balanced chemical equation. If Avogadro number N A , is changed from 6.022 × 1023 mol 1 to 6.022 × 10 20 mol 1, this would change (a) the mass of one mole of carbon (b) the ratio of chemical species to each other in a balanced equation (c) the ratio of elements to each other in a compound (d) the definition of mass in units of grams. Then write a balanced equation for each reaction. An Activity Series is provided at the end of the Background section. Use uppercase for the first character in the element and lowercase for the second character. Examples: Fe, Au, Co, Br, C, O, N, F. Ionic charges are not yet supported and will be ignored. For the reactions involving solid reactants (#2, 4, 5, 7, 11, 13), use the large test tubes. Aqueous zinc nitrate + aqueous lithium chloride, Hydrobromic acid + solid magnesium sulfite, Aqueous rubidium hydroxide + perchloric acid, Aqueous lithium chromate + aqueous gold(III) iodide. Consider Reactions 3 and 14 studied in this lab. Old substances are converted to new substances, which have unique physical and chemical properties of their own. C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) 51 Determine the mass of CO2 produced when 9.0 grams of glucose completely reacts with 9.6 grams of oxygen to produce 5.4 grams of water. Here \(AB\) is an acid (consisting of \(H^+\) and \(X^-\) aqueous ions) and \(BC\) is a base (consisting of \(M^+\) and \(OH^-\) ions). Identify the reaction type – single or double displacement, using the guidelines outlined thus far. aqueous lead(II) nitrate + aqueous potassium chloride. However, one of the products could also be carbonic acid (\(\ce{H2CO3}\)) or sulfurous acid (\(\ce{H2SO3}\)). The limiting reactant in a reaction: a. has the lowest coefficient in a balanced equation. Click here to let us know! If you determine that a reaction will occur, write the correct formula(s) of the products after the arrow. 12 meq of NaOH were required to reach end point.

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