(b) If you take a 10.0-mL portion of the stock solution and dilute it to a total volume of 0.500 L, what will be the concentration of the final solution?

(a) How many milliliters of a stock solution of 6.0 M HNO₃ would you have to use to prepare 110 mL of 0.500 M HNO₃?

(b) If you dilute 10.0 mL of the stock solution to a final volume of 0.250 L, what will be the concentration of the diluted solution?

medical lab is testing a new anticancer drug on cancer cells. The drug stock solution concentration is 1.5 * 10-9 M, and 1.00 mL of this solution will be delivered to a dish containing 2.0 * 105 cancer cells in 5.00 mL of aqueous fluid. What is the ratio of drug molecules to the number of cancer cells in the dish?

Calicheamicin gamma-1, C55H74IN3O21S4, is one of the most potent antibiotics known: one molecule kills one bacterial cell. Describe how you would (carefully!) prepare 25.00 mL of an aqueous calicheamicin gamma-1 solution that could kill 1.0 * 108 bacteria, starting from a 5.00 * 10-9M stock solution of the antibiotic.

Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g/mL at 25 C. Calculate the molarity of a solution of acetic acid made by dissolving 20.00 mL of glacial acetic acid at 25 C in enough water to make 250.0 mL of solution.

(a) What volume of 0.115 M HClO₄ solution is needed to neutralize 50.00 mL of 0.0875 M NaOH?

(b) What volume of HCl is needed to neutralize 2.87 g of Mg(OH)₂?

(c) If 25.8 mL of an AgNO₃ solution is needed to precipitate all the Cl^- ions in a 785-mg sample of KCl (forming AgCl), what is the molarity of the AgNO₃ solution?

(d) If 45.3 mL of a 0.108 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution?

(a) How many milliliters of 0.120 M HCl are needed to completely neutralize 50.0 mL of 0.101 M Ba(OH)₂ solution?

(b) How many milliliters of 0.125 M H₂SO₄ are needed to neutralize 0.200 g of NaOH?

(c) If 55.8 mL of a BaCl₂ solution is needed to precipitate all the sulfate ion in a 752-mg sample of Na₂SO₄, what is the molarity of the BaCl₂ solution?

(d) If 42.7 mL of 0.208 M HCl solution is needed to neutralize a solution of Ca(OH)₂, how many grams of Ca(OH)₂ must be in the solution?

The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide according to: CH3COOH1aq2 + NaOH1aq2¡ H2O1l2 + NaCH3COO1aq2 If 3.45 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00-qt sample of this vinegar?

A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide?

A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (b) What is the identity of the alkali metal cation: Li⁺, Na⁺, K⁺, Rb⁺, or Cs⁺?

An 8.65-g sample of an unknown group 2 metal hydroxide is dissolved in 85.0 mL of water. An acid–base indicator is added and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 56.9 mL of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide? (b) What is the identity of the metal cation: Ca²⁺, Sr²⁺, or Ba²⁺?

A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO₄. (a) Write the balanced chemical equation for the reaction that occurs.

A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO_4. (b) What precipitate forms?

A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO₄. (e) What is the concentration of each ion that remains in solution?

A solution is made by mixing 1.5 g of LiOH and 23.5 mL of 1.000 M HNO₃. (b) Calculate the concentration of each ion remaining in solution.

A solution is made by mixing 1.5 g of Sr(OH)₂ and 23.5 mL of 1.000 M HNO₃. (c) Is the resulting solution acidic or basic?

A 0.5895-g sample of impure magnesium hydroxide is dissolved in 100.0 mL of 0.2050 M HCl solution. The excess acid then needs 19.85 mL of 0.1020 M NaOH for neutralization. Calculate the percentage by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution.

A 1.248-g sample of limestone rock is pulverized and then treated with 30.00 mL of 1.035 M HCl solution. The excess acid then requires 11.56 mL of 1.010 M NaOH for neutralization. Calculate the percentage by mass of calcium carbonate in the rock, assuming that it is the only substance reacting with the HCl solution.

Uranium hexafluoride, UF₆, is processed to produce fuel for nuclear reactors and nuclear weapons. UF₆ can be produced in a two-step reaction. Solid uranium (IV) oxide, UO₂, is first made to react with hydrofluoric acid (HF) solution to form solid UF₄ with water as a by-product. UF₄ further reacts with fluorine gas to form UF6. (a) Write the balanced molecular equations for the conversion of UO₂ into UF₄ and the conversion of UF₄ to UF₆. (b) Which step is an acid-base reaction?

The accompanying photo shows the reaction between a solution of Cd(NO₃)₂ and one of Na₂S. (b) What ions remain in solution?