An alternative way of preparing the imidazolium buffer involves preparing solutions of imidazole (A) and imidazolium (HA; supplied by the manufacturer as a hydrobromide salt with a molar mass of 149g mol) and then combining the solutions ta.obtain a buffer with the desired pH and concentration. Calculate the mass (g) of imidazole (A) and imidazolium (HA) needed to prepare 100ml of the 1.0M stock solutions. Include 1 digit to the right of the decimal. mass HA (g) mass A (g) =

An alternative way of preparing the imidazolium buffer involves preparing solutions of imidazole (A) and imidazolium (HA; supplied by the manufacturer as a hydrobromide salt with a molar mass of 149g mol) and then combining the solutions ta.obtain a buffer with the desired pH and concentration. Calculate the mass (g) of imidazole (A) and imidazolium (HA) needed to prepare 100ml of the 1.0M stock solutions. Include 1 digit to the right of the decimal. mass HA (g) mass A (g) =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH₃COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Based on the information provided, set up a RICE/ICE Table to answer the question. Let x represent the original concentration of CH₃COOH in the water.
A student makes 100.0 mL of a 0.100 M solution of HNO2. What mass (in grams) of NaNO2 should the student add to the solution to make a buffer that buffers at a pH of 4.25. (Hint: use the Henderson-Hasselbalch equation to find the molarity, then find the number of moles required to achieve that concentration in 100.0 mL of solution.)
A 1.0 liter solution contains 0.745 M hydrogen fluoride (HF) and 0.786 M sodium fluoride (NaF). What is the pH of this solution? (Ka for HF is 7.2 x 10 –4) How many moles of solid sodium acetate would have to be added to 2.0 L of 0.293 M acetic acid solution to achieve a buffer of pH 4.77? Assume there is no volume change. Ka for HC2H3O2 is 1.8 × 10 –5 What molar ratio of sodium acetate to acetic acid, is required to create a buffer solution having a pH of 4.58 at 25°C? Ka for HC2H3O2 is 1.8 × 10 –5.
A buffer solution is formed by adding 0.150 moles of solid strontium acetate, Sr(C₂H₃O₂)₂, to 500.0 ml of 0.400 M acetic acid, HC₂H₃O₂ solution. You may assume that the change in volume is negligible upon addition of the solid.Calculate the pH of the buffer solution.Calculate the pH of the buffer solution after the addition of 7.50 ml of 2.00 M NaOH. Acetic Acid: pKa = 4.75 Ka=1.76E-5 M.w.=60.05 g/mol
1. A buffer is formed by mixing 65.0 mL of 0.82 M acetic acid (CH3CO2H) with 80.0 mL of 0.64 M sodium acetate (CH3CO2Na). (a) What is the pH of the solution? Assuming no change in volume, determine the pH of the buffer after (b) addition of 0.0050 mols NaOH; (c) addition of 0.0050 mols HCl. (Kp of NH3 = 1.8 x 10-5) а. b. с. 2 A 22 0O ml samnle of o 0 240 M HCI 0200 VK O
A buffer contains 0.035 mol of boric acid (pKa = 9.15) and 0.015 mol of sodium borate per liter. (a) Calculate the pH of the buffer.(b) Calculate the pH when 2.5 mL of 0.50 M HCl is added to 0.5 L of the buffer.(c) Calculate the pH when 2.5 mL of 0.50 M HCl is added to 0.5 L of pure water.
A buffer is made using 100.0 mL of 0.100 M CH3 CH2 COOH (propanoic acid) and 100.0 mL of 0.100 M NACH3 CH2 COO (sodium propanoate). A) Explain in your own words what will occur (at the molecular level) when an nitric acid is added to the buffer? What would be the effect on the pH? B) Explain in your own words what will occur when LIOH is added tot he buffer? What would be the effect on the [H+]?
A buffer is composed of 0.200 M HC2H3O2 (Ka = 1.8 × 10–5) and 0.250 M NaC2H3O2. What is the pH of the resulting solution after 0.0200 mol of KOH are added to 500.0 mL of the buffer? Assume that the change in volume is negligible. Enter your response in pH units to the nearest 0.01.
A 1.451.45 L buffer solution consists of 0.1590.159 M butanoic acid and 0.3320.332 M sodium butanoate. Calculate the pH of the solution following the addition of 0.0620.062 moles of NaOHNaOH. Assume that any contribution of the NaOHNaOH to the volume of the solution is negligible. The ?aKa of butanoic acid is 1.52×10−51.52×10−5.
Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH₃COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. I've seen a few similar problems solved on here, but mine is asking me to set up an ICE table and then solve for Ka, and I don't understand why I'm supposed to do that.
Imagine that a 50.0 mM MES buffer is made by dissolving an appropriate mass of solid MES in water, adding NaOH ("titrating") until 60.0% of the MES is converted to its conjugate base, then diluting to the required final volume Write the net ionic equation for the reaction that occurs when a little HCl is added to this buffer, then calculate the pH that results when 1.00 mL of 0.250 M HCI is added to 50.0 mL of buffer Calculate the pH that results when 1.00 mL of 0.250 M NaOH is added to 50.0 mL of this buffer. Why does the pH change more when you add NaOH then when you add the same amount of HCI? Calculate the pH that results when 5.00 mL of 0.250 M NaOH is added to 50.0 mL of this buffer.
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