A 75.0 mL of a 0.125 M solution of the protonated form of glycine was titrated with 112.5 mL of 0.125 M NaOH. Find the pH if the pK_a values for the first and second dissociations are 2.34 and 9.78 respectively.

The diagrams below show the different stages of titration for a weak diprotic acid H₂X(aq) with KOH(aq). For simplicity, water molecules and K⁺ ions are not shown. Identify the solution that has the highest pH and the solution that has the lowest pH.

A 25.0 mL sample of 0.080 M (CH₃)₃N (K_b = 6.4×10^–5) is titrated with 0.040 M HBr solution. What is the pH after 15.0 mL of the titrant has been added?

Calculate the pH at the equivalence point for the titration of a 50.0 mL sample of 0.125 M NH₃ with 0.120 M HCl.

What is the pH of the solution of 15.0 mL of 0.113 M trimethylamine titrated with 20.0 mL of 0.156 M HNO₃?

In an experiment, 50.0 mL of 0.200 M HCl is titrated with 0.400 M KOH.
a) Calculate the initial moles of HCl present in the solution.
b) Calculate the volume of 0.400 M NaOH required to reach the equivalence point.
c) Determine the pH of the solution at the equivalence point.
d) Identify the pH titration curve for this experiment.

A 0.115 M HI solution is used to titrate two separate base samples: A 20.00 mL 0.145 M LiOH solution and a 25.00 mL 0.150 M CH₃CH₂NH₂ solution. Which of the two titration curves will have a higher pH at the start?

What is the pH of the following two-component solution?
10.00 mL of 0.134 M NaOH solution and 12.50 mL of 0.128 M HBr solution

The correct K_sp expression for Cd₃(AsO₄)₂ is:

Identify the compound that has the smallest K_sp value from the following general ionic compounds and their molar solubilities in pure water.

Which compound, M₂X or MX₃, would have the lower molar solubility? The K_sp for both is 8.1×10^–6.

Determine whether the pH will change or not in the following scenarios. If the pH changes, identify whether it will increase or decrease.

A. NaBr is added to an HBr solution

B. C₆H₅NH₃Cl is added to a C₆H₅NH₂ solution

C. NaCN is added to an HCN solution

Ni(OH)₂ is a sparingly soluble hydroxide. Will its solubility increase, decrease, or remain unchanged when a small amount of HBr is added to a solution of Ni(OH)₂?

Write a balanced net ionic equation for the dissolution reaction (if it takes place).