State the physical quantity corresponding to the following unit.

$$\mathrm{ng}$$

Select the key term that corresponds to the following definition.

a. aqueous solution (aq)

b. Avogadro’s number

c. Avogadro’s theory

d. combined gas law

e. density

f. directly proportional

g. empirical formula

h. ideal gas constant

i. ideal gas law

j. inversely proportional

k. law of conservation of mass

l. law of definite composition

m. limiting reactant

n. mass/mass percent (m/m %)

o. molarity (M)

p. molar mass (MM)

q. molar volume

r. mole

s. mole ratio

t. molecular formula

u. standard temperature and pressure (STP)

v. stoichiometry

______ the mass of 1 mole of substance expressed in grams

State the physical quantity corresponding to the following unit.

$$\mathrm{kcal}$$

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 $1.05 \mathrm{~g} / \mathrm{mL}$.)