Questions from General Chemistry

Q: Calculate the pH of each of the following solutions of strong acids

Calculate the pH of each of the following solutions of strong acids. a. 1.21 * 10-3 M HNO3 b. 0.000199 M HClO4 c. 5.01 * 10-5 M HCl d. 0.00104 M HBr

Q: Calculate the hydrogen ion concentration, in moles per liter, for

Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pH values. a. pH = 9.01 b. pH = 6.89 c. pH = 1.02 d. pH = 7.00

Q: An oil spill spreads out on the surface of water, rather

An oil spill spreads out on the surface of water, rather than dissolving in the water. Explain why.

Q: Ksp for magnesium carbonate, MgCO3, has a value 3.

Ksp for magnesium carbonate, MgCO3, has a value 3.5 * 10-8 at 25 °C. Calculate the solubility of magnesium carbonate in mol/L and g/L at 25 °C.

Q: What is the effect on the equilibrium position if an exothermic reaction

What is the effect on the equilibrium position if an exothermic reaction is carried out at a higher temperature? Does the net amount of product increase or decrease? Does the value of the equilibrium...

Q: Which component of a buffered solution consumes added strong base? Using

Which component of a buffered solution consumes added strong base? Using your example from Exercise 60, show how this component would react with added NaOH.

Q: The amount of nickel(II) present in an aqueous solution

The amount of nickel(II) present in an aqueous solution can be determined by precipitating the nickel with the organic chemical reagent dimethylglyoxime [CH3C(NOH)C(NOH)CH3, commonly abbreviated as “D...

Q: Which of the following combinations would act as buffered solutions?

Which of the following combinations would act as buffered solutions? a. HCl and NaCl b. CH3COOH and KCH3COO c. H2S and NaHS d. H2S and Na2S

Q: Many metal ions are precipitated from solution by the sulfide ion.

Many metal ions are precipitated from solution by the sulfide ion. As an example, consider treating a solution of copper(II) sulfate with sodium sulfide solution: CuSO4(aq) + Na2S(aq)...

Q: Calcium oxalate, CaC2O4, is very insoluble in water. What

Calcium oxalate, CaC2O4, is very insoluble in water. What mass of sodium oxalate, Na2C2O4, is required to precipitate the calcium ion from 37.5 mL of 0.104 M CaCl2 solution?