A 0.500M solution of a weak acid has a pH of 2.251. a. What is the pKa of the weak acid?

If a weak acid has a pKa value of 5.78, what is the value of Ka for the acid?    Remember to use the rules for significant figures in reporting your answer. There are two fields to input your answer:  Input the number followed by the power of ten to which the number is raised. Ka =  X 10^  Ka= blank X 10^ blank

A scientist needs to prepare an acetate buffered solution at pH 5.0. What is the final concentration of acetic acid (pKa 4.76) and sodium acetate she needs in the solution to have a create a final concentration of 25 mM? The answers are  [Acetic acid] = 9.12 mM [acetate] = 15.88 mM but I do not know how to get to those answers.

A buffer solution contains a weak acid, HA, and its conjugate base, A. The buffer solution has a pH of 5.56, and the weak acid has a pK₂ of 5.00. Without performing a calculation, determine the relationship between the concentration of the weak acid and the concentration of the conjugate base in this buffer solution? O [HA] > [A] O [HA] = [A] O [HA] < [A] The relationship between [HA] and [A] cannot be determined.

An analytical chemist is titrating  57.7mL  of a  0.2900M  solution of formic acid  H2CO2  with a  0.9700M  solution of  KOH . The  pKa  of formic acid is  3.74 . Calculate the pH of the acid solution after the chemist has added  7.03mL  of the  KOH  solution to it.   Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of  KOH  solution added.   Round your answer to  2  decimal places.

Acetic acid (pKa = 4.75) is contained in vinegar.  1. Calculate the pH of an 0.1500 M aqueous solution of acetic acid. 2. What is the pKb of the conjugate base of acetic acid, the acetate anion? 3. Calculate the pH of the solution prepared by mixing 0.0500 mol of acetic acid with 0.0150 mol of sodium acetate in a 500.0 mL volumetric flask.

Calculate the pH of a buffer solution consists of 0.10 M acetic acid and 0.15 M sodium acetate. Suppose 10.0 mL of 0.02 M HCl solution is added to 90.0 mL of HO buffer system. Calculate the final pH. (pKa = 4.74)

A biochemist has 100 mL of a 0.1 M solution of a weak acid with a pKa of 6.3. She adds 6 mL of 1.0 M HCl, which changes the pH to 5.7. Calculate the pH of the original solution. original solution pH:

An analytical chemist is titrating 154.7mL of a 0.2900M solution of dimethylamine CH32NH with a 0.3400M solution of HNO3. The pKb of dimethylamine is 3.27 . Calculate the pH of the base solution after the chemist has added 155.7mL of the HNO3 solution to it. Round your answer to 2 decimal places.

Calculate the pH values and draw the titration curve for the titration of 500 mL of 0.010 M acetic acid (pKa 4.76) with 0.010 M KOH. Part A Calculate the pH of the solution after 0 mL of the titrant have been added. Express your answer to two decimal places. VE ΑΣΦ pH = Submit Part B pH = Request Answer Calculate the pH of the solution after 250 mL of the titrant have been added. Express your answer to two decimal places. VE ΑΣΦ Submit Request Answer Part C = ? ? Calculate the pH of the solution after 450 mL of the titrant have been added. Express your answer to two decimal places.