You add 100.0 mL of 0.10 M KOH to 50.0 mL of 0.20 M HCIO. What is the pH of the resulting solution? Ką for HCIO = 3.5x10-8 O A. 1.17 О В. 4.32 ОС. 9.68 O D. 12.89

What is the pH of a solution containing a mixture of 0.50 M HCN and 0.040 M NaCN?  (Ka = 4.9 x 10-10 for HCN ).

HCN is a weak acid with a Ka = 4.90 x 1010. A 50.00 mL sample of this HCN solution (0.250M) is titrated with 0.500 M NaOH. What is the pH of the original HCN solution?

Calculate the pH of a solution formed by adding 6.00 grams of solid sodium formate, NaCHO₂, to 200.0 ml of 0.400 M formic acid solution, HCHO₂. You may assume that the salt dissolves completely and that the change in volume is negligible upon addition of the solid.pH = ___

25.00mL of a 0.100 M sodium hydroxide is added to 45.00 mL of a 0.100 M acetic acid solution. The Ka of acetic acid is 1.8x10-5. What is the pH of the solution after adding NaOH?

A buffer solution is 0.416 M in H2 S and 0.245 M in NaHS. If K21 for H2S is 1.0 x 10-7, what is the pH of this buffer solution? pH =| A buffer solution is 0.376 M in N.HSO3 and 0.390 M in Na,SOg. If K, for HSO3 is 6.4 × 10-8, what is the pH of this buffer solution? pH =

17. Determine the pH of the resulting solutions when the following reagents are mixed. a. 20.00mL of 0.2500M HCI mixed with 35.00mL of 0.2250M NaOH b. 18.00mL of 0.3500M HC2H;O2 mixed with 15.00mL of 0.3000M NaOH 22.50mL of 0.2000M NH, mixed with 25.00mL of 0.1000M HCI d. 25.00mL of 0.1000M HCIO, mixed with 25.00mL of 0.1000M KOH e. 15.00mL of 0.1000M CH3NH2 mixed with 25.00mL of 0.1500M HCI

Hh.129.

10. One characteristic of blood that we rarely give a thought to is its pH. The pH of blood must be held remarkably constant, varying only by a few hundredths of a pH unit from 7.36 to 7.40.  Blood pH is kept constant primarily through the buffering action of the bicarbonate ion, HCO3-, and dissolved carbon dioxide, commonly represented as H2CO3. The second ionization is negligible in blood so that H2CO3 can be treated as a monoprotic acid.  A) If the Ka1 for H2CO3 is 4.2 * 10-7, what ratio of HCO3- to H2CO3 is necessary to produce a buffer of pH 7.40? B) What is the pH of a buffer that is 1.0 M NaHCO3 and 1.0 M H2CO3? C) If you have 1.00 L of the buffer described above (1.0 M NaHCO3 and 1.0 M H2CO3) and 10.0 mL of 0.100 M HCl is added to it, what is the new pH? D) Just to prove that the buffer helps minimize changes in pH, calculate the pH of a solution prepared by adding 10.0 mL of 0.1 M HCl to 1.00 L of pure water.

8. A 0.0320M solution of a weak base has a pH of 9.45. Determine the Kp of this weak base.