Q: A student needs to calculate the molarity of a solution. If 10.0 grams of NaCl are dissolved in enough water to make 500.0 mL of solution, what is the molarity? (Molar mass of NaCl = 58.44 g/mol)

$$ M = \frac{10.0\ \text{g}}{58.44\ \text{g/mol}} \div 0.500\ \text{L} = 0.342\ \text{mol/L} $$

Q: A patient receives 250 mL of a 0.90% (w/v) NaCl solution intravenously. How many grams of NaCl does the patient receive?

$$ 0.90\ \text{g/100 mL} \times 250\ \text{mL} \div 100\ \text{mL} = 2.25\ \text{g} $$

Q: A gas sample has a volume of 2.00 L at 1.00 atm and 300 K. What will the volume be at 2.00 atm and 300 K, assuming the amount of gas remains constant?

$$ V_2$ = \frac{P_1$ V_1$}{P_2$} = \frac{1.00\ \text{atm} \times 2.00\ \text{L}}{2.00\ \text{atm}} = 1.00\ \text{L} $$

Q: A solution is prepared by dissolving 5.00 g of glucose ($$ \text{C}_6\text{H}_{12}\text{O}_6 ) in $$enough water to make 100.0 mL of solution. What is the molarity of the solution? (Molar mass of glucose = 180.16 g/mol)

$$ M = \frac{5.00\ \text{g}}{180.16\ \text{g/mol}} \div 0.1000\ \text{L} = 0.278\ \text{mol/L} $$

Q: Which of the following functional groups is present in all amino acids?

Amino group ($$ -\text{NH}_2 ) $$and carboxyl group ($$ -\text{COOH} )$$

Q: A sample of gas occupies 3.00 L at 27°C and 1.00 atm. What will be the volume at 127°C and 1.00 atm? (Assume ideal gas behavior.)

$$ V_2$ = V_1$ \times \frac{T_2$}{T_1$} = 3.00\ \text{L} \times \frac{400\ \text{K}}{300\ \text{K}} = 4.00\ \text{L} $$

Question 1

Which of the following best describes the primary focus of CHEM 110 as outlined in the syllabus?

Accepted Answer

A survey of chemistry topics relevant to nursing and allied health sciences, including general, organic, and biochemistry.

Question 2

A student needs to calculate the molarity of a solution. If 10.0 grams of NaCl are dissolved in enough water to make 500.0 mL of solution, what is the molarity? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$$ M = \frac{10.0\ 	ext{g}}{58.44\ 	ext{g/mol}} \div 0.500\ 	ext{L} = 0.342\ 	ext{mol/L} $$

Question 3

Which of the following is the correct IUPAC name for the compound with the formula $$ 	ext{Na}_2	ext{SO}_4 $$?

Accepted Answer

Sodium sulfate

Question 4

A patient receives 250 mL of a 0.90% (w/v) NaCl solution intravenously. How many grams of NaCl does the patient receive?

Accepted Answer

$$ 0.90\ 	ext{g/100 mL} 	imes 250\ 	ext{mL} \div 100\ 	ext{mL} = 2.25\ 	ext{g} $$

Question 5

Which of the following statements about acids and bases is correct according to the Brønsted-Lowry definition?

Accepted Answer

An acid is a proton donor and a base is a proton acceptor.

Question 6

A gas sample has a volume of 2.00 L at 1.00 atm and 300 K. What will the volume be at 2.00 atm and 300 K, assuming the amount of gas remains constant?

Accepted Answer

$$ V_2$ = \frac{P_1$ V_1$}{P_2$} = \frac{1.00\ 	ext{atm} 	imes 2.00\ 	ext{L}}{2.00\ 	ext{atm}} = 1.00\ 	ext{L} $$

Question 7

Which of the following best describes the function of a buffer solution in the human body?

Accepted Answer

It resists changes in pH when small amounts of acid or base are added.

Question 8

Which of the following is the correct Lewis structure for methane ($$ 	ext{CH}_4 $$)?

Accepted Answer

A central carbon atom with four single bonds to four hydrogen atoms, each hydrogen having no lone pairs.

Question 9

A solution is prepared by dissolving 5.00 g of glucose ($$ 	ext{C}_6	ext{H}_{12}	ext{O}_6 ) in $$enough water to make 100.0 mL of solution. What is the molarity of the solution? (Molar mass of glucose = 180.16 g/mol)

Accepted Answer

$$ M = \frac{5.00\ 	ext{g}}{180.16\ 	ext{g/mol}} \div 0.1000\ 	ext{L} = 0.278\ 	ext{mol/L} $$

Question 10

Which of the following functional groups is present in all amino acids?

Accepted Answer

Amino group ($$ -	ext{NH}_2 ) $$and carboxyl group ($$ -	ext{COOH} )$$

Question 11

A sample of gas occupies 3.00 L at 27°C and 1.00 atm. What will be the volume at 127°C and 1.00 atm? (Assume ideal gas behavior.)

Accepted Answer

$$ V_2$ = V_1$ 	imes \frac{T_2$}{T_1$} = 3.00\ 	ext{L} 	imes \frac{400\ 	ext{K}}{300\ 	ext{K}} = 4.00\ 	ext{L} $$

Question 12

Which of the following best explains why water is a polar molecule?

Accepted Answer

Water has a bent molecular shape and an unequal distribution of electrons due to the difference in electronegativity between hydrogen and oxygen.

Question 13

Which of the following laboratory safety practices is most important when working with concentrated acids?

Accepted Answer

Always add acid to water, not water to acid.

Question 14

A buffer solution is made by mixing acetic acid ($$ 	ext{CH}_3	ext{COOH} ) $$and sodium acetate ($$ 	ext{CH}_3	ext{COONa} ). $$What happens to the pH if a small amount of HCl is added?

Accepted Answer

The pH decreases only slightly because the buffer neutralizes the added acid.

Question 15

Which of the following is the correct balanced equation for the combustion of propane ($$ 	ext{C}_3	ext{H}_8 $$)?

Accepted Answer

$$ 	ext{C}_3	ext{H}_8 + 5\ 	ext{O}_2 ightarrow 3\ 	ext{CO}_2 + 4\ 	ext{H}_2	ext{O} $$

Question 16

Which of the following best describes the role of enzymes in biological systems?

Accepted Answer

Enzymes act as biological catalysts, speeding up chemical reactions without being consumed.

Question 17

A solution has a pH of 4. What is the concentration of hydronium ions ($$ [	ext{H}_3	ext{O}^+] ) in $$the solution?

Accepted Answer

$$ [	ext{H}_3	ext{O}^+] = 10$$^{-4}$$\ 	ext{M} $$

Question 18

Which of the following is a correct statement about isotopes?

Accepted Answer

Isotopes of an element have the same number of protons but different numbers of neutrons.

CHEM 110: Elements of General Chemistry – Course Overview and Success Guide

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