Question

2. Does a precipitate of silver chloride form when 200.0 mL of 1.0 x 10-4 M AgNO3 (aq) and 900.0 mL of 1.0 x 10-6 M KCl (aq) are mixed at 25oC?[ Ksp AgCl @ 25oC = 1.6 x 10-10]

Answer 1

Calculate the pH of a NaOH solution of concentration 0.5M (Kw = 1.0 x 10-14 mol2dm-6 at 25oC)

Answer 2

You want to compare Ksp with Qsp.
(AgNO3) = 1E-4 x (200/1100) = ?M
(KCl) = 1E-6 x (900/1100) = ?M
Qsp = (Ag^+)(Cl^-) = ?
If Qsp > Ksp a ppt forms.
If Qsp < Ks no ppt forms.

Answer 3

5. Consider the following reaction: CO2 (g) + H2 (g) CO (g) + H2O (g)
Calculate the value of the equilibrium constant, Kc, for the above system, if 0.1908 moles of CO2, 0.0908 moles of H2, 0.0092 moles of CO, and 0.0092 moles of H2O vapour were present in a 2.00 L reaction vessel at equilibrium.

Answer 4

You should post each question separately. Some won't answer posts that too long; i.e., consists of several questions.
<b>Calculate the pH of a NaOH solution of concentration 0.5M (Kw = 1.0 x 10-14 mol2dm-6 at 25oC) </b>

(H^+)(OH^-) = Kw.
Substitute and solve for (H^+) [note that (OH^-) = (NaOH)], then pH = -log(H^+)

Answer 5

<b>5. Consider the following reaction: CO2 (g) + H2 (g) CO (g) + H2O (g)
Calculate the value of the equilibrium constant, Kc, for the above system, if 0.1908 moles of CO2, 0.0908 moles of H2, 0.0092 moles of CO, and 0.0092 moles of H2O vapour were present in a 2.00 L reaction vessel at equilibrium. </b>

I don't understand your problem with this. Substitute those numbers into the Kc. You want to substitute molarities; i.e., = mols/L. The moles are given; the volume is 2 L.