How many milliliters of 0.105 M HCl are needed to reach the equivalence point of a sample containing 17.8 mL of 0.118 M NH3?

A 1.00 L solution saturated at 25 °C with calcium oxalate (CaC2O4) contains 0.0061 g of CaC2O4. Calculate the Ksp for this salt at 25 °C.

What is the normality, N, of a 0.300 M solution of Ca(OH)2?

Consider the reaction B(aq) + H2O(l) BH+(aq) + OH-(aq). If the salt of HB+(aq) is added, how is the concentration of B(aq) affected?

In determining the total solids in tap water, I found 0.034 g of solids left after evaporating 65 mL of tap water. What is the concentration of solids in the tap water expressed in ppm?

A cell has a standard cell potential of +0.177 V at 298 K. What is the value of the equilibrium constant for the reaction if n = 3 where R = 8.314 J/K-mol and F = 96,488 J/V-mol?

If the equilibrium constant for a two-electron redox reaction at 298 K is 1.5 x 10-4, calculate the corresponding E°. Given R = 8.314 J/K-mol and F = 96,488 J/V-mol.

Which of the following equations is the balanced reduction half reaction for Ag+(aq) + Fe(s) → Fe2+(aq) + Ag(s)?

What is the oxidation of a pure element?

Predict whether the equivalence point for a titration of NH3 with HCl will be above, below, or at pH 7.0.