General Chemistry 2

Rank the following in terms of acidity: HClO, IOH, and HBrO. Explain the trend.

Rank the following in terms of acidity: HClO, HClO$_2$, HClO$_3$, HClO$_4$. Explain the trend.

Rank the following in terms of basicity:

HCN K$_a$ = 4.8 x 10$^{-10}$

HSO$_4^-$ K$_a$ = 1.2 x 10$^{-2}$

HS$^-$ K$_a$ = 7.1 x 10$^{-15}$

H$_2$CO$_3$ K$_a$ = 4.3 x 10$^{-7}$

The percent ionization of NH$_3$ is found to be 4.2% in a solution, find the concentration of NH$_3$.

NH$_3$ (aq) + H$_2$O $\leftrightharpoons$ NH$_4^+$ + OH$^-$ , K$_b$ = 1.8 x 10$^{-5}$

Calculate the pH of a 0.2 M solution of NH$_4$Br, K$_a$ = 5.6 x 10$^{-10}$

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$_4^{3-}$.

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.

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.

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

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

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$^{-12}$

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$^{-8}$

N$_2$ (g) + 3 H$_2$ (g) $\leftrightharpoons$ 2 NH$_3$ (g)

For the reaction above, what is the sign and value of entropy for the reaction, given:

H$_2$ (g), S$^\circ$(at 25$^\circ$C) = 130.7 J/(mol*K)

N$_2$ (g), S$^\circ$(at 25$^\circ$C) = 191.56 J/(mol*K)

NH$_3$ (g), S$^\circ$(at 25$^\circ$C) = 192.77 J/(mol*K)

N$_2$ (g) + 3 H$_2$ (g) $\leftrightharpoons$ 2 NH$_3$ (g)

For the reaction above, calculate the change in free energy for the reaction, if it were to go to completion.

Assign oxidation numbers for the species below. Determine which species is the oxidizing agent and which is the reducing agent. Which species is being oxidized? Which species is being reduced?

Cr$^{3+}$ + Pb $\longrightarrow$ Cr + Pb$^{2+}$

A voltaic cell is constructed using a Cd/Cd$^{2+}$ half cell and a Sn$^{2+}$/Sn half cell. Write out the balanced equation, determine E$^\circ$, and calculate the cell potential at 25$^\circ$C if [Cd$^{2+}$] = 0.50 M and [Sn$^{2+}$] = 0.30 M.

Identify the number of protons, neutrons, electrons, the atomic number, and the mass number for $^{35}_{17}$Cl$^{-1}$