A volume of 500.0 ml. of 0.100 M NaOH is added to 525 mL of 0.250 M weak acid (K, = 4.44 x 10-5). What is the pH of the resulting buffer? HA(aq) + OH (aq) H,O(1) + A (aq) pH =

Calculate the molar solubility (aq., 20 oC) of aluminum hydroxide, Al(OH)3, in 0.000852 M NaOH. The Ksp of Al(OH)3is 2.0 x 10–32.

Annette and Marilyn are given four reactions involving acids and bases. A dark arrow facing left (B -->) means the reaction favours the reactants. A dark arrow facing right ( Products L(aq) + HM(aq) HM(aq) +R (aq) HN(aq) + M¯(aq) HL(aq) + N(aq) Based on this information, the girls determine the correct list of BASES from strongest to weakest as: a. R¯(aq) L-(aq) N-(aq) M-(aq) b. N-(aq) M-(aq) R-(aq) L¯(aq) c. L'(aq) R-(aq) M-(aq) N-(aq) d. M (aq) N-(aq) R (aq) L (aq)

A buffer solution contains 0.35 mol of arsenous acid (H3ASO3) and 0.62 mol of sodium dihydrogen arsenite (NaH₂AsO 3) in 4.40 L. The K₂ of arsenous acid (H3ASO3) is K₂ = 5.1e-10. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.22 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition of 0.18 mol of HI? (assume no volume change) PH =

You prepare a MOPS buffer by adding 0.10 mol MOPS to water then adding 0.040 molNaOH and diluting to a final volume of 500. mL.Calculate the pH of this buffer   C7H14NO3SOH (aq) + NaOH (aq) → C7H14NO3SO− (aq) + Na+ (aq) + H2O (l)

A volume of 500.0 mL of 0.170 M NaOH is added to 535 mL of 0.200 M weak acid (K₁ = 3.14 x 10-5). What is the pH of the resulting buffer? HA(aq) + OH(aq) → H₂O(1) + A (aq) - pH = X10 TOOLS

A volume of 500.0 mL of 0.110 M NaOH is added to 585 mL of 0.200 M weak acid (Ką = 2.92 × 10-5). What is the pH of the resulting buffer? HA(aq) + OH¯(aq) – H,O(1) + A¯(aq) pH =

Give the expression for the solubility product constant for AgCl, based on the following dissolution equation:  AgCl(s)  Ag+(aq) + Cl-(aq).

What is the solubility of silver oxide, Ag₂O, in a solution buffered at pH 10.50? The equilibrium is Ag2O(s) + H₂O(1) 2Ag+ (aq) + 2OH(aq); Ke = 2.0 × 10-8 g/L Solubility: =

Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, andarsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equationCaCO_3(s) ⇌ Ca^2+(aq) + CO3^1−(aq). Is Kc > 1, < 1, or ≈ 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation3Ba^2+(aq) + 2PO_4^3−(aq) ⇌ Ba_3(PO_4)_2(s). Is Kc > 1, < 1, or ≈ 1? Explain your answer.