Which of the following salts, each of which has a solubility product constant (Ksp) equal to 1.0 \times 10 ^ {- 6} has the lowest molar solubility? The correct answer according to the Key is A) MX. Please explain. A) MX B) MX_2 C) MX_3 D) M_2X E) M_2X_3

Im trying to solve for x. is there a better way to solve for x without factoring? Im bad attaht and always mess it up during tests

1 2 3 NEXT > A solution is prepared with 0.55 M HNO₂ and 0.75 M KNO₂. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. -2x 0.75 - 2x [0] 0 [0.55-x] 0.55 +x HNO₂(aq) + [0.55] [0.55 + 2x] 0.55 0.55-x Ka = 0.75 [0.75] [0.55 - 2x] H₂O (1) 0.55 + 2x Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. [6.8 x 10-4] [0.75 +x] 6.8 x 10-4 0.55-2x 2 The Ka for this solution of HNO₂ is 6.8 x 10-4. Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the…

3) Molar solubility and common ions What is the molar solubility of silver chloride in 7.9 mM NaCl(aq)? a. Molar solubility 1.51e-4 mol/L b. How many times is the solubility of silver chloride greater in pure water than in the above NaCl solution? 3 Evaluate Change Problem Values a. Incorrect. You may use an ICE table to find the molar solubility. What are the initial concentrations of the ions present?