Chapter 20, Problem 2ASA

The slightly soluble salt Strontium iodate, Sr(IO3) 2 , dissolves in water as follows: Sr(IO3)2 = Sr2+ + 2 IO3. The solubility is 1.3 grams per liter (g/L). What is the value of Ksp? (Note: this compound is not found in your Ksp table.) Ο 1.8 x 05 O 2.6 x 10-8 О8.8 х 10-6 O 8.8 О 1.1 х 10-7

The solubility product constant for a certain metal phosphate, M3(PO4)2 is Ksp = 5.2 × 10−27. Its molar mass is ℳ = 324.38 g/mol. What is its solubility in g/L? Report your answer to TWO significant figures. Enter your answer in scientific notation using the appropriate boxes. Remember, a number like 1.6, in scientific notation is 1.6 × 100. Note: Your answer is assumed to be reduced to the highest power possible.

The solubility product constant for a certain metal phosphate, M3(PO4)2 is Ksp = 2.1 × 10−27. Its molar mass is ℳ = 279.04 g/mol. What is its solubility in g/L? Report your answer to TWO significant figures. Enter your answer in scientific notation using the appropriate boxes. Remember, a number like 1.6, in scientific notation is 1.6 × 100.

Construct the reaction table for mixing 52.0 mL of 0.110 M AgNO3 and 88.0 mL of 0.180 M K₂CrO4. See the Solubility Product Constant Table. Enter the net ionic equation. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) chemPad → Help X₁X² =+ 2AgNO3(aq) + K₂CrO4(aq) → Ag₂ (CrO4) (s) + 2KNO3(aq) 2AgNO_3(aq) + K_2CrO_4(aq) --> Ag_2(CrO_4)(s) + 2KNO_3(aq) Your answer does not indicate a reaction equilibrium where one exists. Reaction Table initial change Greek final 4.0 5.72 4.0✔ cation 4.0 (a) What mass of precipitate forms? 4.0✔ g mmol mmol mmol + 4.0 15.8 4.0✔ anion 4.0✔ mmol mmol mmol (b) What is the concentration of the excess reactant at equilibrium? (Please answer to 3 sig figs, even if your question version has 2 sig figs.) M 4.0✔ 4.00 4.0✓ precipitate 4.0✔ mmol mmol mmol (c) What is the concentration of the limiting reactant at equilibrium? (The answer is NOT zero. Please use Ksp to calculate this.) 4.0 M

Aluminum in the Al3 + form can be precipitated as Al (OH) 3, adding ammonia to an aluminum solution, but the precipitate is usually gelatinous and difficult to filter. Precipitation from a homogeneous solution provides a more filterable precipitate. The reaction used in this process is the hydrolysis of urea: (image attached) Suppose this reaction occurs in a 100.00 mL solution with an initial Al3 + concentration of 1.50x10-3 mol / L. How many moles of urea must be hydrolyzed to supply enough hydroxide to stoichiometrically combine Al3 + and form the precipitate Al (OH) 3?

Write the balanced molecular chemical equation for the reaction in aqueous solution for cesium carbonate and magnesium nitrate. If no reaction occurs, write NR. CS2CO3 + Mg(NO3)2 →2 CSNO3 + M9CO3 04 02+03+ 4+ 3 6. 7 8. 6. 0. 口3||□4 Os 19 10 (s) (1) (g) (aq) Mg Mn N NR Cs 69°F O pe here to search 4- 2.

Consider the reaction: Al(NO3)3 (aq) + MgCl2 (aq) ➝ AlCl3 (aq) + Mg(NO3)2 (aq). You mix together 25.0 mL of 0.85 M Al(NO3)3 and 25.0 mL of 0.90 M MgCl2 in the lab. What will the final concentration of aluminum chloride be?

(LO 4H, 4K, 4N) Classify the type of chemical reaction for Oboth redox and combustion acid-base combustion Ⓒredox combination CH3OH (1) + 2O2(g) → CO₂ (g) + 2H₂O(g)

Which of the units could be used to quantify the concentration of a solution of CuCl2CuCl2 M % mL g M·s–1