Which salts will be more soluble in an acidic solution than in pure water? CuBr Sn(OH)2 RbClO4 CaSO4 AIPO4

A 0.453 g sample of a diprotic acid is dissolved in water and titrated with 0.200 M NaOH. What is the molar mass of the acid if 34.8 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol 10 11 16 17 18 19 20 21 22 23 24 5

What is [OH – ] in a solution of 0.125 M CH 3 NH 2 and 0.130 M CH 3 NH 3 Cl?      I do not understand how to solve for Kb. Can you please explain this problem step by step?

Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka= 1.5 × 10−6) is titrated with 0.10 M NaOH solution. The ionization of HA in water occurs as the following.HA (aq) + H2O(l) ⇌ A-(aq) + H3O+ (aq)The neutralization reaction between HA and NaOH can be expressed as the following. HA (aq) + NaOH (aq) ® NaA (aq) + H2O (l)  What will be the pH of the HA solution after the addition of 20.0 mL of 0.10 M NaOH to the solution? What will be the pH of the HA solution after the addition of 25.0mL of 0.10M NaOH to the solution?

Which of the following statements are TRUE of buffer solutions? 1. A buffer solution can be made by mixing equal concentrations of acetic acid and sodium acetate. 2. A buffer solution can be made by mixing equal concentrations of hydrochloric acid and sodium chloride. 3. A buffer solution resists changes in pH when small quantities of acid or base are added. O 1 and 2 only O 2 and 3 only O 1 and 3 only All of 1, 2, and 3 O None of these responses åpply.