What volume of 3.51 M KOH is required to prepare 211.0 mL of 0.750 M KOH? a. 1.24 × 10–2 mL b. 5.55 × 102 mL c. 80.2 mL d. 45.1 mL e. 9.87 mL

Chemistry A 76.0 mL portion of a 1.30 M solution is diluted to a total volume of 238 mL. A 119 mL portion of that solution is diluted by adding 177 mL of water. What is the final concentration? Assume the volumes are additive.

Calculate the volume of a 0.0450 M HBr solution that is required to neutralize 120. mL of 0.0200 M Mg(OH)2.2HBr + Mg(OH)2 MgBr2 + 2H2O   A. 53.2 mL   B. 148 mL   C. 107 mL   D. 74.0 mL   E. 37.8 mL

According to Henry’s law the atmospheric partial pressure of CO2 dictates the concentration of aqueous CO2 according to the following equilibrium expression where k is the Henry’s law constant for CO2.  CO2 (g) <-> CO2 (aq)  k=1x10^-1.5  The acid dissociation constant Ka for carbonic acid applies to CO2 (aq). Given pKa1=6.35 and pKa2=10.33 and the fact that the partial pressure of CO2 in the atmosphere is 10^-3.5 atm, find the pH of water in equilibrium with the atmosphere.

What volume of water must be added to 742 mL of a 4.5 M HCI to diluted it to 0.8 M? 4.25 L 1.65 L 4173.8 mL 3431.8 mL 3.92 L

You are given a stock concentration of ADH. The molecular weight of ADH is 35,000 g/mol.  a. What is the molarity of a 54 mg/ml stock solution of ADH? b. you dilute an ADH stock. The concentration is listed below. What is the molarity of a solution made from 78ul of 0 mM stock solution in 17 ml final volume?

1. 100.0 mL of a 0.500 M solution of KBr is diluted to 500.0 mL. What is the new concentration of the solution? 2.100.0 mL of a 0.885 M solution of KBr is diluted to 500.0 mL. What is the new concentration of the solution? 3.If 0.250 L of a 9.70 M HNO3 solution is diluted to 2.00 L, what is the molarity of the new solution?

1. What is the mass of the solution when 50.0 mL of 1.0 M HCI solution is mixed with 50.0 mL of 1.0 M NaOH solution? (d = 1.02 g/mL )

If 10.0 mL of a 3.00 M H2SO4 stock solution are diluted with water to a final volume of 0.500 L, what will be the final concentration of H2SO4 in the dilute solution?   Report your result in decimal notation and to the proper number of significant figures. All numbers are measured.   a) 0.0300 Mb) 0.300 Mc) 0.150 Md) 0.0600 Me) 0.600 M

6. A 25.00 mL aliquot of concentrated hydrochloric acid (11.7 M) is added to 175.00 mL of 3.25 M hydrochloric acid. a. Is this a dilution? b. Determine the number of moles of hydrochloric acid from the 175.00 mL of 3.25 M hydrochloric acid. C. Determine the number of moles of hydrochloric acid in the solution after the addition of the concentrated hydrochloric acid. Assume the volumes are additive. d. Determine the molarity of the solution after the addition of the concentrated hydrochloric acid. Assume the volumes are additive.