Calculatıng the pH of a weak base titrated with a strong acid Jalidt V An analytical chemist is titrating 104.1 mL of a 0.1200M solution of propylamine (C,H,NH,) with a 0.2600M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 53.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH =

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

For a buffer initially containing .08 mol of benzoic acid (HC7H5O2) and .12 mol of C7H5O2 in 1.0 L, what is the pH after .07 mol of OH is added to the buffer? .07 mol OH- .08 mol HC,H,O2 .12 mol C,H¿0; O 4.57 O 5.47 O 2.91 O 4.37 O 3.71

4. What is the pH at each of the following points in the titration of 25.00 mL of 0.100 M CH,CH;COOH with 0.100 M NaOH? a) before the addition of any NaOH; b) after the addition of 10.00 mL of 0.100 M NaOH; c) after the addition of 12.50 mL of 0.100 M NaOH; d) after the addition of 25.00 mL of 0.100 M NaOH; e) after the addition of 26.00 mL of 0.100 M NaOH.

2. Suppose 1.44 0.150 M benzoic acid solution. Calculate the pH of the resulting buffer solution as- suming the volume of the solution does not change on addition of the solid. of sodium benzoate, Na+C,H3COO-, is added to 100.0 mL of the

1000 mL of a buffer solution contains 0.275 moles of HCN, and 0.175 moles of NaCN. Ka of HCN = 6.2 x 10^-10.a) calculate the initial pH b) calculate the pH of the buffer after the addition of 27.5 L of 1.0 M of HCl. c) what is the change in pH of the solution if the same amount of Hcl which was used in part (b) were added to 1000 mL 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+]?

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An analytical chemist is titrating 185.8 mL of a 1.200M solution of benzoic acid (HC,H,CO,) with a 1.200M solution of KOH. The p K, of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 196.6 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. olo pH = ] Ar G Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility ............................... .................................. .............. .... .