Chapter 13a Concentration

2 g =

• 200 mg

• 2,000,000 μg

• 2,000 μg

• 20 mg

750 mg =

• 7.5 g

• 75,000 μg

• 7,500,000 μg

• 0.75 g

27 μg =

• 27,000,000 g

• 2,700 mg

• 0.27 mg

• 0.000027 g

0.25 M CuSO₄ =

Molarity (mol L^-1) to g L^-1

(multiply by molar mass)

1 M NaCl = 1 x 58.5 = 58.5 g L^-1

• 39.9 g L^-1

• 27.9 g L^-1

• 14.6 g L^-1

• 31.9 g L^-1

27 g L^-1 NH₃ =

g L^-1 to % m/v (g/100 mL)

(divide by 10)

58.5 g L^-1 NaCl = 58.5 ¸ 10 = 5.85 % m/v

• 2.7 % m/v

• 27 % m/v

• 17 % m/v

• 1.6 % m/v

0.075 M Pb(NO₃)₂ =

Molarity (mol L^-1) to ppm (mg L^-1)

(multiply by molar mass and then multiply by 1,000)

1 M NaCl = 1 x 58.5 x 1,000 = 58,500 mg L^-1 = 58,500 ppm

• 24,800 ppm

• 20,190 ppm

• 21,240 ppm

• 17,790 ppm

0.062% m/v H₂SO₄ =

% m/v to ppm

(multiply by 10,000 ie. multiply by 10 to get g L^-1 and then multiply by 1,000 to get mg L^-1)

5% m/v HCl = 50,000 ppm

• 620 ppm

• 62 ppm

• 62,000,000 ppm

• 6,200 ppm

2.5 g of CaCO₃ dissolved in 200 mL of water has a concentration of

• 0.125 M

• 0.000 125 M

• 0.184 M

• 0.000 184 M

0.125 mol of SO₂ dissolved in 0.250 L of water has a concentration of

• 0.5 M

• 0.03125 M

• 0.000 5 M

• 0.032 M

5 mL of ethanoic acid added to 95 mL of water has a concentration of

• 5% v/v

• 0.83 M

• 52.6 mL L^-1

• 50 g L^-1