If 1.12 liter of carbon dioxide gas at STP is dissolved in 75.0 milliliters of aqueous solution, what is the number of carbon dioxide molecules dissolved in solution?

a. $2.39 \times 10^{22}$ molecules

b. $3.01 \times 10^{22}$ molecules

c. $4.17 \times 10^{23}$ molecules

d. $1.20 \times 10^{25}$ molecules

e. $1.51 \times 10^{25}$ molecules

State the physical quantity corresponding to the following unit.

$${ }^{\circ} \mathrm{C}$$

State the physical quantity corresponding to the following unit.

$$\mathrm{s}$$

State the physical quantity corresponding to the following unit.

$$\mathrm{cm}^3$$

State the physical quantity corresponding to the following unit.

$$\mathrm{kg}$$

State the physical quantity corresponding to the following unit.

$$\mathrm{cm}$$

The president of a college reports to a board of trustees, and three vice-presidents report to the college president. The chief financial officer reports directly to the board of trustees. Draw a concept map for the college administration.

The chloride in an aqueous sample of $\mathrm{BaCl}_2$ is precipitated with $50.0 \mathrm{~mL}$ of $0.100 \mathrm{M} \mathrm{AgNO}_3$. The excess silver nitrate is titrated with $17.0 \mathrm{~mL}$ of $0.125 \mathrm{M} \mathrm{K}_2 \mathrm{CrO}_4$. Calculate the mass of the barium chloride in the sample.

$$\mathrm{BaCl}_2(a q)+2 \mathrm{AgNO}_3(a q) \rightarrow 2 \mathrm{AgCl}(s)+\mathrm{Ba}\left(\mathrm{NO}_3\right)_2(a q)$$

$$2 \mathrm{AgNO}_3(a q)+\mathrm{K}_2 \mathrm{CrO}_4(a q) \rightarrow \mathrm{Ag}_2 \mathrm{CrO}_4(s)+2 \mathrm{KNO}_3(a q)$$

A sample of sodium carbonate is treated with $50.0 \mathrm{~mL}$ of $0.345 \mathrm{M} \mathrm{HCl}$. The excess hydrochloric acid is titrated with $15.9 \mathrm{~mL}$ of $0.155 \mathrm{M} \mathrm{NaOH}$. Calculate the mass of the sodium carbonate sample.

$$\mathrm{Na}_2 \mathrm{CO}_3(s)+2 \mathrm{HCl}(a q) \rightarrow 2 \mathrm{NaCl}(a q)+\mathrm{H}_2 \mathrm{O}(l)+\mathrm{CO}_2(g)$$

$$\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{NaCl}(a q)+\mathrm{H}_2 \mathrm{O}(l)$$

What is the molar chloride ion concentration resulting from mixing of $50.0 \mathrm{~mL}$ of $0.100 \mathrm{M}$ sodium chloride and $25.0 \mathrm{~mL}$ of $0.100 \mathrm{M}$ potassium chloride?

What is the molar sodium ion concentration resulting from mixing of $50.0 \mathrm{~mL}$ of $0.100 \mathrm{M}$ sodium chloride and $50.0 \mathrm{~mL}$ of $0.200 \mathrm{M}$ sodium sulfate?

The volume of the oceans is $1.4 \times 10^{21}$ liters. Calculate the mass of chlorine in all seawater given the mass percent concentration of chloride ion is $1.90 \%$. (Assume the density of seawater is $1.05 \mathrm{~g} / \mathrm{mL}$.)

Seawater contains approximately $1.22 \times 10^{10}$ atoms of gold per milliliter. How many kilograms of seawater must be evaporated to obtain $12.0 \mathrm{~g}$ of gold? (Assume the density of seawater is $1.05 \mathrm{~g} / \mathrm{mL}$.)

Given that $36.5 \mathrm{~mL}$ of $0.266 \mathrm{M}$ calcium acetate react with $25.0 \mathrm{~mL}$ of $0.385 \mathrm{M}$ sodium carbonate according to the unbalanced equation:

$$\mathrm{Ca}\left(\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2\right)_2(a q)+\mathrm{Na}_2 \mathrm{CO}_3(a q) \rightarrow \mathrm{CaCO}_3(s)+\mathrm{NaC}_2 \mathrm{H}_3 \mathrm{O}_2(a q)$$

What is the mass of $\mathrm{CaCO}_3$ precipitate formed?