Question

5. In part D, there are two sources of Ca2+ in the solution. The first part...

5. In part D, there are two sources of Ca2+ in the solution. The first part of the Ca2+ comes from the CaCl2 solution and the other comes from the Ca(OH)2 dissolved from the original solid.

a.) Determine the Ca2+ amount that came from the CaCl2 solution concentration.

b.) Determine the Ca2+ amount for the dissolved Ca(OH)2 contribution (remember from the chemical equation and equilibrium that for the dissolved Ca(OH)2 the [Ca2+]=1/2[OH].

The concentration of CaCl2 solution is 0.010M CaCl2 . We used 1g of Ca(OH)2.

Homework Answers

Answer #1

a)

One mole CaCl2 contains one mole Ca2+ and 2 moles Cl- ions.

CaCl2   ------> Ca2+ + 2 Cl-

So, the concentration of Ca2+ is equal to the concentration fo CaCl2.

Therefore, the amount of Ca2+ that came from 0.010 M CaCl2 is 0.010 M.

(b)

One mole Ca(OH)2 contains one mole Ca2+ and 2 moles OH- ions.

Ca(OH)2   -----> Ca2+ + 2 OH-

So, the number of moles of Ca2+ is equal to the number of moles of Ca(OH)2.

Moles of Ca(OH)2  = mass of Ca(OH)2 / molar mass of Ca(OH)2

= 1 g/ (74.093 g/mol)

= 0.0135 mol

So, the number of moles of Ca2+ is 0.0135 mol.

Mass of Ca2+ = moles of Ca2+ x atomic mass of Ca

= 0.0135 mol x (40.078 g/mol)

= 0.54 g

Therefore, the amount of Ca2+ is 0.54 g.

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
1. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved Ca(OH)2...
1. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved Ca(OH)2 solid on the bottom of the test tube. If you add an additional scope of Ca(OH)2 to this solution will the concentration of [OH-] in the solution increase, decrease, of be unchanged? (Briefly explain and assume we let the solution reach equilibrium again) 2. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved Ca(OH)2 solid on the bottom of...
Did increasing the starting concentration of Ca2+ in part II of this experiment increase or decrease...
Did increasing the starting concentration of Ca2+ in part II of this experiment increase or decrease the amount of Ca(IO3)2 that dissolved. Explain your answer using the concepts of LeChatelier’s Principle.
You are given a solution that is 0.032 in Cu2+ and 0.032 in Ca2+ that you...
You are given a solution that is 0.032 in Cu2+ and 0.032 in Ca2+ that you wish to separate using selective ion precipitation with OH- ions. The Ksp value for Cu(OH)2 = 4.80 X 10-20 and the Ksp value for Ca(OH)2 = 5.02 X 10-6. The two metal hydroxides used to set the pH threshold for the separation is Ca(OH)2 b) What is the threshold pH, below which you get precipitation of the least soluble metal hydroxide while the most...
A 0.4505 g sample of CaCO3 was dissolved in the HCl and the resulting solution diluted...
A 0.4505 g sample of CaCO3 was dissolved in the HCl and the resulting solution diluted to 25.00 mL in a volumetric flask. A 25.00 mL aliquot of the solution required 29.25 mL of EDTA solution for titration to the Eriochrom Black T end point. a. How many moles of CaCO3 were present in the solid sample? b. What is the molar concentration of Ca^2+ are contained in a 250.00 mL aliquot of the CaCl2 solution? c. How many moles...
The hydroxide ion concentration, [OH-], in each of your trials can be calculated from the concentration...
The hydroxide ion concentration, [OH-], in each of your trials can be calculated from the concentration of the hydrochloric acid, 0.050 M HCl, and the volume of both the HCl and Ca(OH)2 used in the titration. According to the net ionic equation (calcium hydroxide, Ca(OH)2 (s), in water) determine the ratio of moles of calcium ion, Ca2+, to moles of hydroxide ion, OH-, in the solution of calcium hydroxide, Ca(OH)2. Using this ratio, determine the molarity of calcium ion in...
a.) What is the molarity of a solution prepared by dissolving 47.1 grams of Ca(OH)2 in...
a.) What is the molarity of a solution prepared by dissolving 47.1 grams of Ca(OH)2 in a total solution volume of 400.0 mL? b.) What volume of the solution in part (a) is required to prepare 5.00 L of 0.100 M Ca(OH)2? c.) The dilute solution in part (b) is used in a titration experiment to neutralize 35.00 mL of an HClO solution. 24.48mL of 0.100 M Ca(OH)2 are required to fully neutralize the hypochlorous acid. Give the balanced chemical...
1. Part A A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2...
1. Part A A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2 in water. The concentration of Ba2+ ion in the solution was found to be 7.52×10?3M . Calculate Ksp for BaF2. Part B The value of Ksp for silver carbonate, Ag2CO3, is 8.10×10?12. Calculate the solubility of Ag2CO3 in grams per liter. 2. The generic metal hydroxide M(OH)2 has Ksp = 9.05×10?18. (NOTE: In this particular problem, because of the magnitude of the Ksp and...
2. What is the pH and [F–]eq in a 0.100 M solution of HF?      Ans....
2. What is the pH and [F–]eq in a 0.100 M solution of HF?      Ans. pH = 2.08; [F–] = 8.2×10–3 M 3. What would happen to the equilibrium [H3O+] and the pH of the solution if we suddenly added some solid NaF? (Remember, sodium salts are completely soluble in water. How will this change affect the equilibrium system? Which direction will the reaction shift to minimize the disturbance?) If we suddenly added some solid NaF the solution will...
When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution...
When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO3(aq)+CaCl2(aq)→2AgCl(s)+Ca(NO3)2(aq) Part A What mass of silver chloride can be produced from 1.94 L of a 0.126 M solution of silver nitrate? Part B The reaction described in Part A required 3.49 L of calcium chloride. What is the concentration of this calcium chloride solution?
Part A The following equation shows the equilibrium in an aqueous solution of ammonia: NH3(aq)+H2O(l)⇌NH4+(aq)+OH−(aq) Which...
Part A The following equation shows the equilibrium in an aqueous solution of ammonia: NH3(aq)+H2O(l)⇌NH4+(aq)+OH−(aq) Which of the following represents a conjugate acid-base pair? The following equation shows the equilibrium in an aqueous solution of ammonia: Which of the following represents a conjugate acid-base pair? NH3 and H2O NH4+ and OH− H2O and OH− NH3 and OH− Part Part B What is the conjugate base of HCO3−? Express your answer as a chemical formula. Part Part C What is the...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT