HomeworkLib
Question

b. MgCl, is dissolved in distilled water at 25°C until the saturated solution is obtained (system reaches equilibrium). The c
Calculate the solubility product, K of MgCl2. Explain the effect of increasing the temperature on the amount of MgCl, Justify
science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

DATE PAGE #tj 2f ২ १%-9) 2 f M al १ -3 xley ठैव = ५४ (१ १5् ४ ।० ) । 4s 3 2 3 १.९५ X1o । ी ন ही alus Hen the duasen c০obldDATE PAGE. 2-f 1-35 x 10M 453 x15X10) 2१.8५ *16 १ Li ileta P2 No dersases Besaue पा readuon tei m bachward Sana ormaon roduct

0 0
Add a comment
Know the answer?
Add Answer to:
b. MgCl, is dissolved in distilled water at 25°C until the saturated solution is obtained (system...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • Barium hydroxide Ba(OH)2 was dissolved in pure water at 5°C until a saturated solution was obtained....

    Barium hydroxide Ba(OH)2 was dissolved in pure water at 5°C until a saturated solution was obtained. The pH of this solution was found to be 12.25. a) What is the molar solubility of Ba(OH)2 in pure water at this temperature? Express your answer in mol/L. Show your work. b) What is the Ksp of Ba(OH)2 at this temperature? Show your work.

  • 1) A saturated solution of copper (II) iodate in pure water has a copper ion concentration...

    1) A saturated solution of copper (II) iodate in pure water has a copper ion concentration of 2.7X10^-3 M. a) whar is the molar solubility of copper iodate in a 0.35 M Potassium iodate solution B) what is the molar solubility of copper Iodate in 0.35 M copper nitrate solution 2) a)consider the slightly soluble salt, silver chloride, Agcl. If you had 10.0 g of silver chloride, what volume of water would be required to completely dissolve this amount b)...

  • Ba(OH)2 was dissolved in pure water at 5 degree celsius until a saturated solution was obtained....

    Ba(OH)2 was dissolved in pure water at 5 degree celsius until a saturated solution was obtained. the pH of this solution was found to be 12.25 a) what is the solubility of Ba(OH)2 in pure water at this temperature? answer in mol/L b) what is the Ksp of the Ba(OH)2 at this temperature?

  • At room temperature, you are given a litre of a solution of PbCl2(aq)inwhich there is excess...

    At room temperature, you are given a litre of a solution of PbCl2(aq)inwhich there is excess PbCl2(s)i.e. a saturated solution. State and explain the effect of the following on the concentration of the Pb2+ ions in the solution? [Remember to use ideas on equilibrium, Le Chatelier's Principle, etc. in your answer] Adding more PbCl2 solid Adding NaClsolid Adding 500 ml of water, assuming there will still be excess solid afterwards. Heating the solution to 35 0C assuming the solubility is...

  • 1. A saturated solution of lead(II) chloride was prepared by dissolving PbCl2 solid in water. The concentration of Pb+2...

    1. A saturated solution of lead(II) chloride was prepared by dissolving PbCl2 solid in water. The concentration of Pb+2 ion in the solution was found to be 1.62*10^-2M . Calculate Ksp for PbCl2 . 2. The value of Ksp for silver chromate, Ag2CrO4 is 9.0*10^-12 . Calculate the solubility of Ag2CrO4 in grams per liter.

  • In a saturated solution of MgF2 at 16 °C, the concentration of Mg2+ is 1.44x10 –3...

    In a saturated solution of MgF2 at 16 °C, the concentration of Mg2+ is 1.44x10 –3 M The equilibrium is represented by the equation MgF2 -->Mg 2+ + 2 F-. A.Write the expression for the solubility product constant, Ksp. B.Calculate the value of Ksp at 16°C for MgF2 Note: Your answer is assumed to be reduced to the highest power possible. C.Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution  at 16°C to which 0.450 mole of...

  • Saturated, Unsaturated & Supersaturated Solutions Solution, in which the concentration of solute is that determined by...

    Saturated, Unsaturated & Supersaturated Solutions Solution, in which the concentration of solute is that determined by its solubility (at given temperature) is called SATURATED solution. One cannot add more solute to such a solution. We also say that a saturated solution is in equilibrium with pure solute: If we add solid Nacl to an already saturated solution of NaCl, that solid remains in equilibrium with dissolved Naci. Solution containing less solute than would be in the saturated solution, is UNSATURATED...

  • Learning Goal: To learn how to calculate the solubility from Kspand vice versa. Consider the following equilibrium be...

    Learning Goal: To learn how to calculate the solubility from Kspand vice versa. Consider the following equilibrium between a solid salt and its dissolved form (ions) in a saturated solution: CaF2(s)⇌Ca2+(aq)+2F−(aq) At equilibrium, the ion concentrations remain constant because the rate of dissolution of solid CaF2 equals the rate of the ion crystallization. The equilibrium constant for the dissolution reaction is Ksp=[Ca2+][F−]2 Ksp is called the solubility product and can be determined experimentally by measuring thesolubility, which is the amount...

  • When silver sulfate (Ag2SO4) is dissolved in water at 25 °C, until saturation is reached, the...

    When silver sulfate (Ag2SO4) is dissolved in water at 25 °C, until saturation is reached, the Ag+ cation equilibrium concentration is 3.0 x 10 ^-5 M. a) Determine the value of the solubility constant for Ag2SO4 (b) Determine the maximum amount (in grams) of AgNO3, a completely water-soluble salt, which can be dissolved in 3.2 L of a H2SO4 solution without precipitating Ag2SO4 Note: Actually the molarity of H2SO4 is not given in the exercise. Is it really necessary for...

  • Part A and Part B. Also question #3-post lab. (its circled) A. Molar Solubility and Solubility Product of Calcium Hydroxide Trial I Trial 3 Trial 2 25.0 1. Volume of saturated Ca(OH), solution (m...

    Part A and Part B. Also question #3-post lab. (its circled) A. Molar Solubility and Solubility Product of Calcium Hydroxide Trial I Trial 3 Trial 2 25.0 1. Volume of saturated Ca(OH), solution (mL) 2. Concentration of standardized HCl solution (molU/L) 3. Buret reading, initial (mL 4. Buret reading, final (mL) 5. Volume of HCI added (mL) 6. Moles of HCI added (mol) 7. Moles of OH" in saturated solution (mol) 8. (OH1, equilibrium (mol/L) 9. (Ca2 ], equilibrium (mol/L)...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT