Chapter 15 Problem Set KEY

After adding the water how was the equilibrium affected? If a compound was removed how? Explain the effect of water addition using Le Chatelier's Principle.

The solubility product expression for La2(CO3)3 is Ksp = __. a) [La3+]3[CO32-]2 b) [La2+]3[CO32-]2 c) [La3+]2[CO32-]3 d) [2La3+]2[3CO32-]3 e) [2La3+][3CO32-]

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For AgOH, Ksp = 1.5 x 10-8. What is the molar solubility of AgOH in a solution containing 0.1 M of NH3 buffered at pH = 7? (K;[Ag(NH3)2')= 1.6 x 107). A. 0.20 M B. 0.025 M C. 0.25 M D. 0.05 M

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An equilibrium reaction between chromate ions, CrO4 2- (yellow), and H+ ions is established to produce dichromate, Cr₂072- (orange). Note the colours. A student adds NaOH to a test tube containing an orange mixture of the above reagents. What is observed? 01. The solution turns from orange to yellow O 2.A precipitate forms 3. The solution tuimns from orange to colourless O4. The solution remains orange

The following is a solubility product expression for Pb(ClO3)4: Ksp= O [Pb4+][CIO3] O [Pb4+][CIO3]4 O [Pb4+][4CIO3-14 O [Pb4+][CIO3] O [Pb4+][CIO3-]¹

Calculate the Ksp for magnesium fluoride if the solubility of MGF2 in pure water is 0.000234 M. a. 5.1 x 10-11 O b.5.8 x 10-5 C. 9.3 x 10-4 d. 1.3 x 10-11

B. Chemical equilibrium using cobalt (II) compounds Test tube #1 Test tube #2 Test tube #3 1. Adding water 1. Adding HCI Pale red red 2. Adding distilled water red 3. placing the test tube in hot water bath dark red 4. placing the test tube in ice bath Pale red 1. Adding distilled water dark red 2. Heating the test tube blue 3. Adding distilled water dark red Part B (Use equations 5.3, 5.4, 5.5, 5.6 and Le Chatelier's principle to explain your answer if needed) Explain what happened when you added water to test tube #1 • Why adding HCI to test tube #2 caused a change? • In step 4, you added water to test tube #2 and a change happened, explain why the colour changed using the equations • Explain how the hot water and ice baths affected test tube #2?

In the above reaction, A is the two reactants, B is the activated complex, and C is the product. This reaction is exothermic.  Which has the highest energy? a. A b. B c. C

15. What is the hydroxide-ion concentration of a saturated solution of Ni(OH)2? For Ni(OH)2, Ksp = 2.0 × 10 15. A. 2.8 x 10M B. 7.9 x 10 M C. 1.0 x 10 M D. 2.7 x 10 M E. 1.6 x 10 M

Assume we are to tackle a complex equilibria problem using the process we learned in class. In this example, we’re going to look at dissolving CuS in water.  The relevant equilibrium reactions are as follows: CuS   ⇋   Cu2+   +   S2–                                                                                                                                   Cu2+   +   OH–   ⇋   Cu(OH)2 S2–   +   H2O   ⇋   HS–   +   OH–                                                                                                           H2O   ⇋   H+   +   OH– HS–   +   H2O   ⇋   H2S   +   OH– Write 1 charge balance equation.

Assume we are to tackle a complex equilibria problem using the process we learned in class. In this example, we’re going to look at dissolving CuS in water.  The relevant equilibrium reactions are as follows: CuS   ⇋   Cu2+   +   S2–                                                                                                                                   Cu2+   +   OH–   ⇋   Cu(OH)2 S2–   +   H2O   ⇋   HS–   +   OH–                                                                                                           H2O   ⇋   H+   +   OH– HS–   +   H2O   ⇋   H2S   +   OH– Write 1 mass balance equation.

11:39 PM Mon May 29 Question 14 of 34 What is the charge of the complex formed by a platinum (II) metal ion coordinated to two ammonia molecules and two chloride ions? Tap here or pull up for additional resources

Using the dissociation constant, Kd 1x1044, calculate the equilibrium concentrations of CN in a 0.333 M solution of Fe(CN)6-. О а. 1.8х10-5 м O b. 3.8x10-4 M O c. 6.0x10-7 M O d. 9.1x10-4 M

When 18.0 mL of a 1.80x10-4 M sodium sulfide solution is combined with 12.0 mL of a 2.87x10-4 M nickel(II) acetate solution does a precipitate form? (yes or no) [Review Topics] Use the References to access important values if needed for this question. For these conditions the Reaction Quotient, Q, is equal to Submit Answer 80 Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support NOV 1 27 MacBook Air * Previous Next> tvill AA H Save and Exit DII

In aqueous solution the Ni" ion forms a complex with four cyanide anions. .2+ Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the last step in the formation of the complex. K, = I Write the Last Step: Last Step: I Don't Know Submit 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility 21 TO FEB tv Aa 14 MacBook Air 888 E10 esc F3 F1 & 3 4 7 E Y T (of

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16. Which is the correct equilibrium-constant expression for this reaction? PCI5(aq) E> PCI3{aq) + Clz{aq) [PCI3][Cl2] [PCl] 1 C. [PCl3] а. [PCI3][Cl2] [PCls] [CL] d. [PCI3] b.

3B. Effect of Temperature: Test tube Color of Temperature Is intensity of red color Increased or Is [Fe(SCN)]? darker or lighter compare to increases or the reference test tube color decreases? solution decreased 1. Reference Blood red color 6. Hot water Light blood Increases bath lighter red color 7. Ice water bath Dark blood Decreases Darker red color Question 15: Using the evidence of a shift in chemical equilibrium in test tube 6, explain the role of temperature in this reaction. Question 16: For test tube 7, complete the equation by adding “heat" to the equation as either a reactant or product. Fe*(aq) + 4 CI (aq) [FeCl4]* (aq)