Answer Happy

If the Ksp of AgCl is 1.7 x 10-10, what is the molar concentration of the chloride ions at equilibrium? The reaction is provided below: + Cl (aq) AgCl (s)→ Ag (a (aq) 3.2 x 104 M. 1.3 x 10-5 M. 0.51 x 10-2 M 07.2 x 10-10 M 0.045 M

Which statement is not true regarding Ksp? the reactant is included in the equilibrium expression because it is a solid the products are in aqueous state of matter O it is an equilibrium reaction the reactant is a solid the products are ions

In a buffer system with 0.025 L each of 0.6 M weak acid and 0.6 M conjugate base, what would be the new amount of total moles of acid in the buffer solution if 0.01 moles of HCI is added? 0.025 O 0.2 0.001 0.005 O 0.7

What is the general solubility product constant equation (Ksp) for BaSO4? Ksp [BaSO4] = O Ksp = [Ba] [SO4]² Ksp = [Ba²+] [SO4²-1 OKsp = [Ba²+] [SO4²-1/[BaSO4] None of the above

EXTRA CREDIT: In a 1L buffer solution made of 0.5 moles of acetic acid and 0.5 moles of sodium acetate, what is the pH if 0.1 moles of NaOH is added as a disturbance to the buffer? Assume pKa for acetic acid is 3.17. 12.1 6.00 3.35 8.87 2.68

Which of the following solutions could impact the ability of MgCO3 to dissolve in solution due to the "common ion effect"? HCI NaCl Na₂CO3 H₂SO4 NaNO3

When 0.2 L of 5 M HCI is titrated with 0.4 L of 2M NaOH, how many moles is in excess of either acid or base? 0.2 moles HCI is in excess 0.8 moles NaOH is in excess 0.8 moles HCI is in excess 0.2 moles NaOH is in excess 1 moles HCI is in excess