If 26.7 mL of 0.106 M acid with a pK₂ of 5.37 is titrated with 0.102 M NaOH solution, what is the pH of the titration mixture at halfway to the equivalence point?

Calculate pH for a weak base/strong acid titration. Determine the pH during the titration of 35.9 mL of 0.286 M methylamine (CH3NH₂, Kp = 4.2x10-4) by 0.286 M HCIO4 at the following points. (a) Before the addition of any HCIO4 (b) After the addition of 13.2 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 54.9 mL of HCIO4

Consider the titration of 25.00mL of 0.200M Methylene (CH3NH2). The titrant is 0.120M HCL. Calculate each of the following. (a) the initial pH of base? (b) the pH of 5.00mL added? (c) the pH at 1/2 the HCl needed to reach equivalence point? (d) the volume of added acid required to reach equilibrium? (e) the pH at equivalence point?

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 chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.

1.Determine the pH during the titration of 62.9 mL of 0.360 M hydrocyanic acid (Ka = 4.0×10-10) by 0.360 M KOH at the following points. (Assume the titration is done at 25 °C.)(a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint)  (d) At the equivalence point  (e) After the addition of 94.4 mL of KOH    2. When a 23.3 mL sample of a 0.379 M aqueous hypochlorous acid solution is titrated with a 0.407 M aqueous sodium hydroxide solution,(1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 32.5 mL of sodium hydroxide have been added?

A chemistry graduate student is given 125. mL of a 0.90M benzoic acid (HC,H,CO2) solution. Benzoic acid is a weak acid with K,=6.3 × 10 °. - 5 What mass of NaC,H,CO, should the student dissolve in the HC,H,CO, solution to turn it into a buffer with pH = 3.97? You may assume that the volume of the solution doesn't change when the NaCH,CO, is dissolved in it. Be sure your answer has a unit symbol, and round it 2. to 2 significant digits. x10

Consider the titration of 25.0 mL of 0.200M CO2H with 0.250M NaOH. How many milliliters of base are required to reach the equivalence point? Calculate the pH at each of the following points. (a) After the addition of 7.0 mL of base (b) Halfway to the equivalence point (c) At the equivalence point (d) After the addition of 25.0 of base

Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 2.00 ✕ 102 mL of solution and then titrate the solution with 0.148 M NaOH. C6H5CO2H(aq) + OH-(aq)  C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2-   M Na+  M H3O+  M OH-  M C6H5CO2-What is the pH of the solution?

A chemistry graduate student is given 300. mL of a 1.60M pyridine (C H,N) solution. Pyridine is a weak base with K,=1.7 × 10 What mass of CH,NHC1 should the student dissolve in the CH,N solution to turn it into a buffer with pH = 5.16? You may assume that the volume of the solution doesn't change when the CH,NHCI is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.