Question

Barium sulfate is only sparingly soluble in water. When excess solid barium sulfate is placed in...

Barium sulfate is only sparingly soluble in water. When excess solid barium sulfate is placed in contact with water to form a saturated solution, the following equilibria are established:

1) BaSO4(s) <---> Ba 2+(aq) + SO4 2-(aq)

2) SO4 2-(aq) + H2O(l) <---> HSO4-(aq) +OH- (aq)

3) 2H2O (l) <---> H3O+(aq) +OH-(aq)

Will the concentration of Ba2+ ion increase, decrease, or remain the same when each of the following is done? Explain your reasoning.

a) solid sodium sulfate is added to the solution

b) several drops of concentrated sodium hydoxide solution are added to the solution (ignore the effect of dilution)

c) additional solid barium sulfate is placed in contact with the solution

Homework Answers

Answer #1

Ans

a)

When sodium sulfate is added into the solution , the amount of sulfate ion in the solution will increase , which will cause less dissociation of barium sulfate in the solution , hence the concentration of Ba2+ will decrease.

b)

When sodium hydroxide is added in the solution , the concentration of hydroxide ions in the solution will increase, which will cause the reaction 2 to move backwards and hence sulfate concentration increases in the solution , causing less dissociation of barium sulfate and then decrease in concentration of Ba2+ ions.

c)

When additional solid barium sulfate is placed in contact with the solution , the equillibrium is moved forward and the Ba2+ concentration in the solution increases.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
To analyze for barium in an unknown white powder, an excess of sodium sulfate solution was...
To analyze for barium in an unknown white powder, an excess of sodium sulfate solution was added to a 0.624 g sample of the powder dissolved in water. A white precipitate of BaSO4 was isolated, dried, and found to weight 0.438 g. What is the mass percent of Ba in the white powder sample? a. 0.267% b. 41.3% c. 58.9% d. 70.2% e. none of the above Write the balanced chemical equation: Show all calculation:
A solution is made by dissolving 15.1 g of barium hydroxide, Ba(OH)2, in enough water to...
A solution is made by dissolving 15.1 g of barium hydroxide, Ba(OH)2, in enough water to make exactly 100. mL of solution. Calculate the molarity of each species: Ba(OH)2 _______ mol/L Ba2+ _________ mol/L OH- _________ mol/L
2. For half-cell B, when NaOH(aq) is added to Cu2+(aq), a sparingly soluble solid, Cu(OH)2, will...
2. For half-cell B, when NaOH(aq) is added to Cu2+(aq), a sparingly soluble solid, Cu(OH)2, will form. a. Write the reaction for the formation of Cu(OH)2. The Ksp for Cu(OH)2 is 4.8 x 10^-20. b. Interpret the magnitude of Ksp. When NaOH(aq) is added to Cu2+(aq), what will happen to the "free" [Cu2+]? Choose one. [Cu2+] will increase [Cu2+] will decrease [Cu2+] will not change cannot be predicted. c. After the nearly insoluble solid forms, the next step in the...
Use the solubility generalizations on the information page to predict if one or more precipitates will...
Use the solubility generalizations on the information page to predict if one or more precipitates will form when aqueous solutions of chromium(III) sulfate (Cr2(SO4)3) and barium acetate (Ba(CH3COO)2) are mixed. Write the formula of any precipitate that could form in one of the blanks. If a box is not needed, leave it empty. If no precipitate is predicted, leave both blanks empty ___________ ... ____________. Soluble Ionic Compounds 1. All sodium (Na+), potassium (K+), and ammonium (NH4+) compounds are SOLUBLE....
1) a. Write the balanced molecular equation that occurs for the complete reaction of sulfuric acid...
1) a. Write the balanced molecular equation that occurs for the complete reaction of sulfuric acid with sodium hydroxide. b. To determine the molarity of your final sulfuric acid solution, you titrate the final solution with a standardized sodium hydroxide solution to the second equivalence point. If 26.32 mL of 0.1000 M sodium hydroxide was required for complete reaction with 10.00 mL of the final sulfuric acid solution, determine the molarity of the final sulfuric acid solution precisely to four...
When 4.50 g of Ba(s) is added to 100.00 g of water in a container open...
When 4.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 54.35°C. If the specific heat of the solution is 4.18 J/(g • °C), calculate ΔH for the reaction, as written. Ba(s) + 2 H2O(l) → Ba(OH)2(aq) + H2(g) ΔH = ? When 4.50 g of Ba(s) is added to 100.00 g of water in a...
13. A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the...
13. A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 97.7-mL sample of this solution was withdrawn and titrated with 0.0687 M HBr. It required 57.8 mL of the acid solution for neutralization. (a) What was the molarity of the Ca(OH)2 solution? _____ M (b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100...
When 2.50 g of Ba(s) is added to 100.00 g of water in a container open...
When 2.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 40.32°C. If the specific heat of the solution is 4.18 J/(g • °C), calculate ΔH for the reaction, as written. Ba(s) + 2 H2O(l) → Ba(OH)2(aq) + H2(g) ΔH = ?
Give the oxidation number for the species or the indicated atom in the following: Cs in...
Give the oxidation number for the species or the indicated atom in the following: Cs in Cs2O ————— Calculate the mass of KI in grams required to prepare 5.00 × 102 mL of a 3.0 M solution —————— A sample of 0.3151 g of an ionic compound containing the bromide ion (Br−) is dissolved in water and treated with an excess of AgNO3. If the mass of the AgBr precipitate that forms is 0.7199 g, what is the percent by...
3) Cerium(IV) sulfate  is used to titrate a solution of iron(II) ions, with which it reacts according...
3) Cerium(IV) sulfate  is used to titrate a solution of iron(II) ions, with which it reacts according to Ce4+(aq) + Fe2+(aq) = Ce3+(aq) + Fe3+(aq) A cerium(IV) sulfate solution is prepared by dissolving 38.14 g of Ce(SO4)2 in water and diluting to a total volume of 1.000 L. A total of 17.82 mL of this solution is required to reach the endpoint in a titration of a 250.0-mL sample containing Fe2+(aq). Determine the concentration of Fe2+ in the original solution. answer:...