General Chemistry 2

Find the concentration of HS$^-$, S$^{2-}$ and H$_3$O$^+$ in a 0.075 M solution of H$_2$S

H$_2$S + H$_2$O $\longrightarrow$ HS$^-$ + H$_3$O$^+$, K$_{a1}$ = 1.0 x 10$^{-7}$

HS$^-$ + H$_2$O $\longrightarrow$ S$^2-$ + H$_3$O$^+$, K$_{a2}$ = 1.0 x 10$^{-19}$

Calculate the pH and concentration of all species of a 3.0 M solution of phosphoric acid, H$_3$PO$_4$

What is the pH of a 0.1 M sulfuric acid solution? (did you know sulphuric is an alternative spelling?)

H$_2$SO$_4$ + H$_2$O $\longrightarrow$ HSO$_4^-$ + H$_3$O$^+$, K$_{a1}$ = 1.0 x 10$^{3}$

HSO$_4^-$ + H$_2$O $\longrightarrow$ SO$_4^{2-}$ + H$_3$O$^+$, K$_{a2}$ = 1.2 x 10$^{-2}$

Calculate the pH of a 5.0 M H$_3$PO$_4$ solution and the equilibrium concentrations of the species H$_3$PO$_4$, H$_2$PO$_4^-$, HPO$_4^{2-}$, and PO$_4^{3-}$.

Find the equilibrium concentrations of the species H$_2$SO$_4$, HSO$_4^-$, SO$_4^{2-}$, and H$^{+}$ given a 1.0 M solution of H$_2$SO$_4$.

Find the pH of the buffer solution consisting of 0.60 M HF and 1.0 M KF (K$_a$ of HF = 7.2 x 10$^{-4}$)

A buffer solution consisting of 0.60 M HF and 1.0 M KF (Ka of HF = 7.2 x 10$^-4$) is titrated by 0.1 mol NaOH. After the NaOH is added, there is 1 L of solution. Find the pH of the solution.

A buffer solution consisting of 0.60 M HF and 1.0 M KF (Ka of HF = 7.2 x 10$^-4$) is titrated by 0.2 mol HCl. After the HCl is added, there is 1 L of solution. Find the pH of the solution.

Find the pH of the buffer solution consisting of 0.100 M HONH$_2$ and 0.100 M HONH$_3^+$ (K$_b$ of HONH$_2$ = 1.1 x 10$^{-8}$), after .02 moles HCl is added to the buffer solution? (assume the final volume of the solution is 1 L)

10.00 mL of an unknown H$_2$CO$_3$ solution is titrated with 0.0500 M NaOH and it requires 15.67 mL to reach the end point. What is the concentration of the H$_2$CO$_3$ ?

H$_2$CO$_3$ + 2 NaOH $\longrightarrow$ Na$_2$CO$_3$ + 2 H$_2$O

Sketch the titration curve for 50.0 mL 0.1 M HCl, K$_a$ = 1.8 x 10$^{-5}$ with 0.1 M NaOH. Include points on your graph for the initial pH, the pH at half way to the equivalence point, the pH at the equivalence point and the pH after the equivalence point.

Sketch the titration curve for 50.0 mL 0.1 M CH$_3$COOH, K$_a$ = 1.8 x 10$^{-5}$ with 0.1 M NaOH. Include points on your graph and an example calculation for the initial pH, the pH at half way to the equivalence point, the pH at the equivalence point and the pH after the equivalence point.

Find the pH of a 0.1 M solution of NH$_3$. If 50 ml of this solution is titrated by 50 ml of 0.1 M HCl, find the pH at the equivalence point. (K$_a$ = 5.56 x 10$^{-10}$ )

By experiment, it is found that of 6.2 x 10$^{-12}$ moles of Pb$_3$(PO$_4$)$_2$ dissolves in 1 L of aqueous solution at 25$^\circ$C. What is the solubility product constant, K$_{sp}$, at this temperature?

Calculate the solubility (in grams per liter) of PbI$_2$ in water from the solubility product constant 1.4 x 10$^{-8}$.

What are the concentrations of the ionic species in a saturated solution of Ag$_2$CrO$_4$

K$_{sp}$ = 1.1 x 10$^{-12}$

Calculate the equilibrium concentration of Pb$^{2+}$, I$^-$, Na(\^+$, and NO$_3^-$when 100.0 mL of 0.0500 M Pb(NO$_3$)$_2## and 200.0 mL of 0.100 M NaI are mixed.

PbI$_2$ K$_{sp}$ = 1.4 x 10$^{-8}$

What is the molar solubility of Ag$_2$CrO$_4$ in 0.100 M AgNO$_3$? Compare this to the molar solubility of Ag$_2$CrO$_4$ in water, 1.3 x 10$^{-4}$ M

Ag$_2$CrO$_4$ K$_{sp}$ = 9.0 x 10$^{-12}$

The concentration of Mg(NO$_3$)$_2$ is 4 x 10$^{-4}$ M and the concentration of NaOH is 2 x 10$^{-4}$, do you expect Mg(OH)$_2$ to precipitate?

Mg(OH)$_2$ K$_{sp}$ = 8.9 x 10$^{-12}$

A solution contains 1.0 x 10$^{-4}$ M Cu$^+$ and 2.0 x 10$^{-3}$ M Pb$^{2+}$. When I$^{-}$ is added, which will precipitate first? How much I$^-$ is needed to cause a precipitate to form?When CuI is added to PbI$_2$

CuI K$_{sp}$ = 5.3 x 10$^{-12}$

PbI$_2$ K$_{sp}$ = 1.4 x 10$^{-8}$