25 C, lanthanum(III) hydroxide has a Ksp of 2.0 x 10^–21. a. Calculate the molar solubility of lanthanum(III) hydroxide. b. Calculate the pH of a saturated lanthanum(III) hydroxide solution. c. Will lanthanum(III) hydroxide precipitate when 0.040 g of solid La(NO3)3 is dissolved in 100 mL of a solution buffered to pH 7.00? Why or why not?

1. A saturated solution of Mg(OH)2 is prepared having a large excess of Mg(OH)2. Sn(NO3)2 is added to the solution. Ksp = 2.0 ✕ 10-11 for Mg(OH)2 and Ksp = 5.3 ✕ 10-26 for Sn(OH)2. a) What [Sn2+] is required to start the precipitation of Sn(OH)2? b) What [Sn2+] is required so that the [Mg2+] in solution will be 0.12 M?   2. Solid NaI is added to a solution which is 0.025 M in TlNO3 and 0.015 M in AgNO3. Assume the volume remains constant. Ksp = 8.9 ✕ 10-8 for TlI and Ksp = 1.0 ✕ 10-16 for AgI. a) Which compound precipitates first TII or AgI?   b) What is the concentration of the first ion precipitated when the second ion starts to precipitate?       3. What is the molar solubility of PbSO4 in 0.19 M MgSO4? Ksp = 1.0 ✕ 10-8 for PbSO4.

Silver and ammonia may react to form Ag(NH₃)₂⁺ complex (K f = 1.66 x 10 7 ). A 500 mL of 0.20mol Ag⁺ and 500 mL of 0.80 mol NH₃ are mixed together.a. Write the complexation reaction.b. Write the formation constant expression.c. What is the concentration of the complex at equilibrium?d. What is the concentration of the metal at equilibrium?

A student measures the molar solubility of barium fluoride in a water solution to be 7.37x10-³ M. Based on her data, the solubility product constant for this compound is _______ A student measures the molar solubility of iron(III) hydroxide in a water solution to be 2.23x10-10 M. Based on her data, the solubility product constant for this compound is ________ A student measures the $²- concentration in a saturated aqueous solution of manganese(II) sulfide to be 7.39x10-8 M. Based on her data, the solubility product constant for manganese(II) sulfide is ______

You dissolve 0.45 g of Cu in 4.0 mL of 12 M HNO3. What mass of solid sodium hydroxide pellets must be added to precipitate the Cu²+ as Cu(OH)2? Calculate the volume of 2.5 M NaOH required to neutralize the unreacted HNO3.

Chemistry 7) The solubility product constant of Mg(OH),2 at 25°C is KP=3.4*10^-11 .In a solution of Mg(NO3)2 0.125M. add NaOH solution. Calculate the pH value for which Mg(OH)2 starts to precipitate.

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In this lab, we will experimentally determine the titration curve for the titration of a weak acid solution against a strong base solution. The weak acid we will use is potassium hydrogen phthalate, KHP, its chemical structure is shown below. KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP–. HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a)  Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b)  Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c)  Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g and at 25 °C has a pKa of 5.4.

A buffer solution contains 0.442 M CH3NH3Cl and 0.294 M CH3NH₂ (methylamine). Determine the pH change when 0.062 mol NaOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change = C Submit Answer 54 $ 998 R F F4 V % 5 [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support G 6 B MacBook Air S Y H & 7 ◄◄ N F7 U J * 8 ►ll F8 I M -0 9 K ►► F9 O -0 L F10 P 4) F11 Previous + Next> = Save and Exit 4))) F12 ( delete

A solution contains 0.21 M Pb^ 2+ and 0.42 M Al ^ 3+ .Calculate the pH range that would allow Al(OH)3 to precipitate but not Pb(OH)2. The Ksp for Al(OH)3 and Pb(OH)2 can be found in this table. A. maximum Ph: B. minimum Ph: