# silver sulfate ksp expression

By definition, the solubility product constant, Ksp, is equal to. a. water b. Unless otherwise noted, LibreTexts content is licensed by CC BY-NC-SA 3.0.

a) 1.4 x 10-5 b) 6.5 x 10-8 c) 2.3 x 10-4 d) 8.1 x 10-9 e) 3.4 x 10-6 Based on our data, we think this question is relevant for Professor Bindell's class at UCF. Silver bromide AgBr 5.0×10 –13. A: The acidity of carboxylic acid is increases, when it contains electron withdrawing group is near in ... Q: How many kilojoules are required to change the temperature of 64.5 g  of water from 22.2 oC  to 45.3... Q: Give equations for the formation and hydrogenolysis of N-benzyloxycarbonyl methionine. What is the molar solubility of silver sulfate in water? What are the ion concentrations in a saturated solution at this temperature? Question.

For our silver sulfate saturated solution, $Ag_2SO_{4 (s)} \rightleftharpoons 2Ag^+_{(aq)} + SO^{2-}_{4(aq)}$, we can write a solubility product constant expression as, $K_{sp} = \dfrac{ [Ag^+_{(aq)}]^2[SO_{4(aq)}^{2-}] }{ [Ag_2SO_{4(s)}] }$. You can use an ICE table to find the equilibrium concentration of the two ions, #" ""Ag"_ color(blue)(2)"SO"_ (4(s)) " "rightleftharpoons" " color(blue)(2)"Ag"_ ((aq))^(+) " "+" " "SO"_ (4(aq))^(2-)#, #color(purple)("I")color(white)(aaaaaacolor(black)(-)aaaaaaaaaaaaaacolor(black)(0)aaaaaaaaaaacolor(black)(0)# Ksp = [Ag+]2 ⋅[SO2− 4] In your case, this will be equal to. Silver chloride AgCl 1.8×10 –10. Answer Save. Step 1. 3 views. All known compounds can be dissolve in certain solvents whereas they remain insoluble in other solvents. As you can see, the molar solubility of the salt decreased as a result of the presence of the silver cations #-># think common-ion effect here. Experts are waiting 24/7 to provide step-by-step solutions in as fast as 30 minutes!*. The Ksp for silver sulfate (Ag2SO4) is 1.2 x 10-5.?

What is the molar solubility of silver sulfate in water? 1 decade ago. (a) NaOH in ... Q: Name two causes of rancidity in oils

A large value of Ksp indicates a soluble substance; for ionic compounds it tells us that there will be many ions in solution.

Step 2: Write the expression for $$K_{sp}$$: Solubility Product Tables that give Ksp values for various ionic compounds are available.

Always begin problems involving Ksp by writing a balanced equation: The question provides us with the concentration of the solution, BaSO4 . Find answers to questions asked by student like you. The Ksp is 1.5x10-5 at 25oC. (Silver(I)). Silver cyanide AgCN 1.2×10 –16. Ksp = (2s)2 ⋅s = 4s3. We need to find the concentration of the individual ions for our equation. How many moles of KOH is required p... A:  We’ll answer the first question since the exact one wasn’t specified. What is acid value of oils? The Ksp is 1.5x10-5 at 25oC. 2 Answers. Problem: The solubility of silver sulfate (MW 311.8) is 4.73 g/L at 25°C. Silver azide AgN 3 2.8×10 –9. Substitute values into the Ksp expression and solve for the unknown: $= (3.90 \times 10^{-5})(3.90 \times 10^{-5})$, Example $$\PageIndex{3}$$: Calculating ion concentrations when Ksp is known. 0.10 M AgNO3 c. 0.20 M K2SO4. 1 We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. We will refer to our equilibrium constant as $$K_{sp}$$, where "sp" stands for "solubility product". check_circle Expert Answer. 62060 views around the world. Remember that polyatomic ions remain together as a unit and do not break apart into separate elements. Eaaaaaa − aaaaaaaaaaaaa2saaaaaaaaaaas. Q: Predict the products obtained from the reaction of triolein with the following reagents. How can you use the solubility product constant to calculate the solubility of a sparingly... What is the molar solubility of magnesium fluoride in a solution that is #"0.1 M"# sodium fluoride? Relevance. Ksp = (2M)^2(M) = 4M^3 = 1.2x10^-5. Recall what we learned about Keq.

Therefore, we will write our solubility product constant expression for our saturated silver sulfate solution as: Please note that it is VERY IMPORTANT to include the ion charges when writing this equation. Plug in your value to find. From Wikipedia, the free encyclopedia Silver sulfate (Ag 2 SO 4) is an ionic compound of silver used in silver plating and as a non-staining substitute to silver nitrate. #"Ag"_ color(blue)(2)"SO"_ (4(s)) rightleftharpoons color(blue)(2)"Ag"_ ((aq))^(+) + "SO"_ (4(aq))^(2-)#, Now, when you dissolve the salt in pure water, the initial concentration of the dissolved ions will be equal to zero. Silver sulfate Ag 2 SO 4 1.4×10 –5. Silver chromate Ag 2 CrO 4 1.1×10 –12. Write the expression for the solubility product constant, Ksp, for Ca3(PO4)2. This sulfate is stable under ordinary conditions of use and storage, though it darkens upon exposure … . $$K_{sp}$$, which again is just a special case of $$K_{eq}$$, provides us with the same useful information: A low value of Ksp indicates a substance that has a low solubility (it is generally insoluble); for ionic compounds this means that there will be few ions in solution. Upon dissolution, Ag2SO4 --> 2Ag+ + SO4--and Ksp = [Ag+]^2 [SO4--], so . Calculate solubility product constant. Silver sulfate, #"Ag"_2"SO"_4#, is considered insoluble in aqueous solution, which implies that a dissociation equilibrium between the dissociated ions and the undissolved solid is established when you dissolve the salt in water. Recall from Section 2.5 - since 1 mole of BaSO4 produces 1 mole of Ba2+ and also 1 mole of SO42-, then . #color(purple)("C")color(white)(aaaaaacolor(black)(-)aaaaaaaaaaacolor(black)((+color(blue)(2)s))aaaaaaacolor(black)((+s))#

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