Consider an amphoterics hydroxide M(OH)2(s), where M is ageneric metal.M(OH)2(s) <---> M2+(aq) +2OH-(aq) Ksp= 8x10-16M3 M(OH)2 (s) + 2OH-(aq) <--->M(OH)42-(aq) Kf= 0.03M-1 Estimate the solubility of M(OH)2 in a solutionbuffered at pH= 7.0, 10.0, & 14.0 ...Please explain indetail

Chemistry

answers

watching

views

23 Nov 2019

Consider an amphoterics hydroxide M(OH)2(s), where M is ageneric metal.
M(OH)₂(s) <---> M²⁺(aq) +2OH^-(aq) Ksp= 8x10^-16M³

M(OH)₂ (s) + 2OH^-(aq) <--->M(OH)₄^2-(aq) Kf= 0.03M^-1

Estimate the solubility of M(OH)₂ in a solutionbuffered at pH= 7.0, 10.0, & 14.0 ...Please explain indetail

answers

watching

views

For unlimited access to Homework Help, a Homework+ subscription is required.

Join us on Discord

Chemistry Study Group

Join now

Related questions

The following data were collected at 20 ^oC for the reaction of bromophenol blue (HBPB^2-) and hydroxide ions (OH^-):

HBPB^2- (aq) + OH^- (aq) ---> BPB^3- (aq) + H₂O (l)

The times required to form a constant [BPB^3-] at varying initial concentrations of reactants were determined and tabulated. From the rate data, determine the rate law for the reaction.

trial	[OH^-]	[HBPB^2-]	reaction time (sec)	rate (1/sec)
1	1.00	7.22 x 10^-6	75
2	0.25	7.22 x 10^-6	290
3	1.00	3.63 x 10^-6	152

		rate = k[HBPB^2-]²[OH^-]
		rate = k[HBPB^2-]²[OH^-]²
		rate = k[HBPB^2-][OH^-]
		rate = k[HBPB^2-][OH^-]²

QUESTION 2

Which of the following balanced molecular equations represent reactions for which the rate law expression could likely be determined via time to turbidity determinations? Select all that apply.

	a.	2 KI (aq) + Pb(NO₃)₂ (aq) ---> PbI₂ (s) + 2 KNO₃ (aq)
	b.	2 HBr (aq) + Ca(OH)₂ (aq) ---> 2 H₂O (l) + CaBr₂ (aq)
	c.	2 NO (g) + 5 H₂ (g) ---> 2 NH₃ (g) + 2 H₂O (g)
	d.	FeS (s) + HCl (aq) ---> FeCl₂ (aq) + H₂S (g)
	e.	3 SrCl₂ (aq) + 2 Li₃PO₄ (aq) ---> Sr₃(PO₄)₂ (s) + 6 LiCl (aq)

QUESTION 3

When working in the laboratory a small amount of 0.30 M sodium thiosulfate accidentally splashes on your exposed forearm. What should you do? Select all that apply.

	a.	Inform your lab instructor.
	b.	Proceed immediately to the sink in the laboratory and flush the area with copious amounts of water. Then wash the area with mild hand soap.
	c.	Leave the laboratory immediately. All lab work is over for you today.
	d.	Do nothing.
	e.	Stop, drop, and roll.

QUESTION 4

	volume of 1.0 M HCl	volume of water	volume of 0.3 M Na₂S₂O₃
well 1	2.0 mL	0	3.0 mL
well 2	2.0 mL	1.5 mL	1.5 mL
well 3	2.0 mL	2.0 mL	1.0 mL

The above table summarizes the amounts and concentrations of the reactants that will be used in each trial in Parts II. Use the dilution equation, M₁V₁ = M₂V₂, to calculate the concentration M_f (molarity_final) of Na₂S₂O₃ in each well after mixing but before any reaction occurs. The [HCl] has been worked for you as an example.

M_1(HCl)V₁ = M_2(HCl)V₂ where V₂ = final total volume V_f

(1.0 M)(2.0 mL) = M_2(HCl)(5.0 mL)

M_2(HCl) = 0.40 M = M_f(HCl)

- a. b. c. d. e. f.	well 1 M_f
- a. b. c. d. e. f.	well 2 M_f
- a. b. c. d. e. f.	well 3 M

a.	0.090 M
b.	0.18 M
c.	0.60 M
d.	0.20 M
e.	0.060
f.	0.30 M

1.Phenolphthalein is, HPhen, is a common acid-base indicator. In solutions it dissociates according to the equation:

Le Châtelier’s Principle 8
HPhen(aq) ---> H+(aq) + Ph-(aq)
clear (HPhen = weak acid) pink (Ph- = conjugate base)
If phenolphthalein is added to distilled water, the solution is clear. If a drop or two of 6 M NaOH is added to the clear solution, it turns bright pink. If to that solution one adds a few drops of 6 M HCl, the color reverts to clear.

a. Give the net ionic equation for the reaction that happens when NaOH is added to phenolphthalein. Why does adding 6 M NaOH to the clear solution of phenolphthalein tend to cause the color to change to pink? (Note that in solution NaOH exists as Na⁺ and OH^- ions.)
b. Give the net ionic equation for the reaction that happens when HCL is added to phenolphthalein. Why does adding 6 M HCl to the red solution tend to make it turn back to clear? (Note that in solution HCl exists as H⁺ and Cl^- ions.)

2. Iron(III) hydroxide is only very slightly soluble in water. The reaction by which it goes into solution is:
Fe(OH₎₃(s) Fe ³⁺(aq) + 3 OH^-(aq)

a. Formulate the expression for the equilibrium constant, Ksp, for the above reaction.
b. Explain why Fe(OH)3 might have very appreciable solubility in 1 M HCl. (Consider the effect of Reaction 2 on the Fe(OH)3 solution reaction.)

burgundycicada286

1.What is the molar solubility of CaCO3 (Ksp = 2.5 x 10^-9) in an aqueous solution where the carbonate ion concentration is 0.30 M at 25Â°C?

2. Two solutions are mixed; one solution contains Al³⁺ and the other solution contains OH^-. If, at the instant of mixing, but before any precipitate forms, [Al³⁺] = 3.2 x 10^-10 M and [OH^-] = 5.6 x 10^-8 M, which of the following statements is true? The Ksp value for Al(OH)3 is 4.6 x 10^-33 at 25Â°C?

No precipitate forms because Qsp > Ksp

A precipitate forms because Qsp > Ksp

No precipitate forms because Qsp < Ksp

A precipitate forms because Qsp < Ksp

3.Which salt is the least soluble in water at 25Â°C?

Which salt is the least soluble in water at 25Â°C?