1. The pH of a buffer solution containing 0.5 mole/litre of CH:COOH and 0.5 mole/litre CH.COONA has been found to be 4.76. What will be the pH of this solution after 0.1 mole/litre HCI has been added to the buffer? Assume that the volume is unchanged. Ka = 1.75 x 105

An analytical chemist is titrating 221.9 mL of a 0.9800M Solution of propionic acid (HC,H,CO,) with a 0.8400OM solution of NaOH. The pK, of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 190.2 mL of the NAOH SOlution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH Solution added. Round your answer to 2 decimal places. pH = ?

5. Suppose 30.0 mL of 0.15 M KOH is added to 50.0 mL of 0.20 MHCIO. What will be the pH of the resulting solution? pKa = 7.52

A 25.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 19.4 mL of NaOH have been added to the acid? Please report 2 decimal places.

25.0 ml of 0.100M NaOH is titrated with HC2H3O2  and 50.0mL of the acid is used to reach the endpoint.              a)Write the chemical equation for the reaction. Include states of matter.  b)Calculate the molarity of the acid HC2H3O2.  c)What is the starting pH for the base in the titration?

An analytical chemist is titrating 231.8 mL of a 0.9900M solution of acetic acid (HCH, CO,) with a 1.200M solution of NaOH. The p K, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 131.2 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. alo pH %3| Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessibility CA

A 1.0-L buffer solution contains 0.100 mol acid, HA, and 0.100 mol base, NaA. The value of K, for the acid HA is 1.8x104. Ignoring the small volume change, what is the most likely pH of the solution if a 10.0 mL- sample of 1.00M HCI is added to the original buffer? O 1.20 < pH < 1.45 O 5.50 < pH < 5.74 O 4.10 < pH < 4.22 O 3.51 < pH < 3.69

An analytical chemist is titrating 68.1 mL of a 0.6500M solution of propionic acid (HC,H,CO,) with a 0.4500M solution of KOH. The p K, of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 114. mL 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.

Calculate the change in pH when 5.00 mL of 0.100 M HC1(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH, (aq) and 0.100 M in NH,Cl(aq). Consult the table of ionization constants as needed. 4 ApH = Calculate the change in pH when 5.00 mL of 0.100 M NAOH is added to the original buffer solution. ApH :

A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3H­O­-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 300.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.) Answer not in scientific notation