In Class Exercise Neutralization Upload 9C Write the balanced equations for the following acid-base neutralization reactions: • Stomach acid and one component of Mylanta: HCI + Mg(OH)2→ Phosphoric acid and baking soda H;PO4 + NaHCO, → In Class Buffers Upload 9D Write out an equation showing what occurs when each of the following is added to this phosphate buffer: a) small amount of HCI (aq) b) small amount of KOH (aq)

In Class Exercise Neutralization Upload 9C Write the balanced equations for the following acid-base neutralization reactions: • Stomach acid and one component of Mylanta: HCI + Mg(OH)2→ Phosphoric acid and baking soda H;PO4 + NaHCO, → In Class Buffers Upload 9D Write out an equation showing what occurs when each of the following is added to this phosphate buffer: a) small amount of HCI (aq) b) small amount of KOH (aq)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 102CWP: Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 ...

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In lab, you will be provided with a 1.8 M acetic acid solution (CH3COOH) and solid sodium acetate trihydrate (NaOOCCH3  3H2O). You want to make 100.0 mL of a 0.5 M acetic acid buffer at pH 5.00. How many grams of sodium acetate trihydrate, and what volume (mL) of the 1.8M acetic acid solution and deionized water should you combine? The pKa of acetic acid is 4.75. Show all work.
Propanoic acid that, along with its sodium salt, can be used to make a buffer that has a pH of 5.25. If you have 512.5 mL of a 0.272 M solution of that acid, how many grams of the corresponding sodium salt do you have to dissolve to obtain the desired pH? For propanoic acid, HC3H5O2, Ka = 1.3 x 10-5. m(salt) = Want solution ASAP
Part 1: A buffer system is set up with [HA] = 0.550 M and [A-] = 0.460 M in 1.0 L of aqueous solution. If pKa = 6.10, what is the pH of the buffer solution? Part 2: To the original buffer solution, what is the pH of the buffer solution after adding in 0.0500 mol of HBr (assume no volume change)? Part 3: To the original buffer solution, what is the pH of the buffer solution after adding in 0.0400 mol of KOH (assume no volume change)?
A buffer solution was prepared by dissolving 0.04 mol Na2HPO4(s) and 0.02 molNaH2PO4(s) in water and diluted to a total volume of 1.0 L. 1. What are the buffering molecules in this solution? Also state whether they act as acid orbase.2. What will be the concentration of the buffer? Report your calculations.3. Calculate the pH of the buffer solution. (K =5*10-8 ). Show your calculations4. How does the pH in the buffer change when 1 mmol NaOH is added? Show calculations.
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A laboratory manager wants to prepare 500.00 mL of a buffer with a pH of 4.471 from equimolar solutions of CH3CO2H (Ka = 1.800e-5) and LiCH3CO2. What volume of the LiCH3CO2 solution would be required? Key Concept: Buffers resist pH change and are prepared by mixing the conjugate acid and base together. The pH is determined from the Henderson-Hasselbach equation: pH = pKa + log([A−]/[HA]).Solution: Since the molarities of the two solutions making the buffer are the same, the Henderson-Hasselbach equation can be written as: pH = pKa + log(V(A−)/V(HA)) where V(A−) = the volume of the conjugate base and V(HA) = the volume of the conjugate acid.
A buffer solution was prepared by dissolving 0.04 mol Na2HPO4(s) and 0.02 molNaH2PO4(s) in water and diluted to a total volume of 1.0 L. 1 What will be the concentration of the buffer? Report your calculations.2 Calculate the pH of the buffer solution. (K =5*10 ). Report your calculations3 How does the pH in the buffer change when 1 mmol NaOH is added? Report your calculations.
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In some natural systems the pH must be maintained within very narrow limits. e.g. in human blood the pH must remain close to 7.4 or cell deterioration occurs. Blood contains several weak acid/conjugate base equilibria called buffers, which control the pH.One weak acid present in blood is the dihydrogen phosphate ion, H2PO4-(aq), for which the equilibrium in aqueous solution is H2PO4-(aq) +H2O(l) <--> HPO42-(aq) + H3O+(aq). a) What would be the effect on this equillibrium of adding hydrochloric acid solution?b) Write the expression for the equilibrium constant of this reaction.c) If 0.5 mol H2PO4- and 0.5 mol HPO42- are in equilibrium in 1.0L of aqueous solution, calculate the pH of the solution. (Ka for H2PO4-= 6.4 x 10-8)d) 0.010 mol HCl is now added to the 1.0L of the solution in c). Assuming that all the added H+ ions are used up in the equilibrium shift, calculate the concentrations of H2PO4- and HPO42-. Hence calcuate the pH of this solution.e) 0.010 mol HCl has been added…
A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The titration requires 30.0 mL of 0.1025 M NaOH. Calculate the molar mass of the acid. (a) Would the molar mass be too high, too low, or unaffected if the student accidentally used 0.1400 g in the calculation? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated (b) Would the molar mass be too high, too low, or unaffected if the student accidentally used 20.0 mL instead of 30.0 mL? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated
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