What is the nickel ion concentration in a solution prepared by mixing 397 ml. of 0.353 M nickel nitrate with 443 ml. of 0.327 M sodium hydroxide? The K of nickel hydroxide is 5.48 x 10 - 16. |N)=

Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s /Csp of 1.1 X 10-,<) gives it such low solubility' that it can be safely consumed. What is the molar solubility' of BaSO4. What is its solubility' in grams per 100 g of water?

An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)

Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?

95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated with hydrogen sulfide gas. For example, nickel(II) precipitates nearly quantitatively as NiS when H2S gas is bubbled through a nickel ion solution. How many milliliters of gaseous H2S at STP are needed to precipitate all (he nickel ion present in 10. mL of 0.050 M NiCl2 solution?

Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?

What volume of 0.250 M NaOH is required to react completely with 0.0100 moles of H2SO4? (a) 80.0 mL (b) 60.0 mL (c) 40.0 mL (d) 125 mL

1.

Consider the following equilibrium: Cu²+ (aq) + 4NH3(aq) Cu(NH3)4²+₁ (aq) (Kf = 4.8e+12) A solution is made by mixing 15.0 mL of 0.90 M CuSO4 and 1.00 L of 0.530 M NH3. Assume additive volumes to answer the following questions. Give all answers to three sig figs. a) What is the concentration of NH3 in the resulting solution? [NH3] = .47 M b) What is the concentration of Cu(NH3)42+ in the resulting solution? [Cu(NH3)4²+] = 5.3e-2 X M c) What is the concentration of Cu²+ in the resulting solution? [Cu²+] = 5.3e-2 X M

A saturated solution of iron(II) oxalate contains 0.0659 g FeC2O4 in 1.00 L of solution. What is the solubility product constant, Ksp? The molar mass of FeC2O4 is 143.87 g/mol. Ksp = [ ? ] x [?] x 102] Do not round until the end. Coefficient (green) Exponent (yellow) Enter