Ksp
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KspQuestions
- How can you use the solubility product constant to calculate the solubility of a sparingly soluble ionic compound?
- Question #f5130
- What is Ksp?
- How can Ksp be calculated?
- How is Ksp related to molarity?
- Question #da59d
- Question #71344
- Question #17cc3
- What is the molar solubility of magnesium fluoride in a solution that is #"0.1 M"# sodium fluoride?
- (a) How much aluminium hydroxide will dissolve in 500ml of water at #25^@C# given that #K_(sp)=3xx10^(-34)#? (b) How much will dissolve in 500ml of a solution of 0.04M #Ba(OH)_2# ?
- Question #ad761
- Question #885cc
- Question #0be3f
- Question #fa00c
- Question #0e38d
- Question #ade43
- In a certain mystery liquid, the compounds #Al_2S_3#, #K_3N#, #Na_2S#, and #RbBr# each have a value of #Ksp = 1.0 xx 10^-10#. Which of these solids should be the least soluble in the mystery liquid? (Choices in answer).
- Question #32388
- Question #32390
- Question #13e47
- Question #b13d6
- Is it true that the GREATER the #"solubility product,"# #K_"sp"#, the more soluble the salt?
- How do we assess the solubilities of various salts in various solutions?
- Question #f53d2
- Solubility of #Mg(OH)_2# is #1.6# x #10^-4# #"mol/L"# at #298# #K#. What is its solubility product?
- Calculate the #pH# at which #Mg(OH)_2# begins to precipitate from a solution containing #0.1# #M# #Mg^(2+)# ions? #K_(sp)# for #Mg(OH)_2# = #1.0# x #10^-11#.
- How much #KBr# should be added to #1# #L# of #0.05# #M# #AgNO_3# solution just to start precipitation of #AgBr#? #K_(sp)# of #AgBr# = #5# x #10^-13#.
- Will a precipitate form when we micx Ca(NO3)2(aq) with NaOH(aq) if the concentrations after mixing are both 0.0175M?
- (1)425ml of a saturated solution of lanthanum iodate, #La(IO_3)_3#, has #2.93 xx 10^-4# mole of #La^(3+)# (a)what is the concentration of #IO_3^-#? (b)calculate the solubility product of lantham iodate?
- After 20.0g of #Na_2SO_4# are added to a 0.5 L saturated solution of #CaSO_4#, does the concentration of #Ca^(2+)# increase, decrease, or stay the same?
- What is solubility and solubility product??
- What is the difference between carbon dioxide, and silicon dioxide? How do we formulate the solubility product for the salt #A_2B_3#
- Question #d71a4
- Question #d893a
- What is the solubility in mol/L of silver iodide, #"AgI"# ?
- How many kilograms of salt (NaCl) can be dissolved in 2 liters of water at 25 degrees Celsius? The solubility product constant, Ksp, is 38.65
- Using the following data, how do you calculate the Ksp value given that the solubility of #"Pb"_3("PO"_4)_2# is #6.2xx10^(-12) "mol/L"# ?
- Jack mixes 82 mL of #4.0x10^-4 M# silver acetate with 18 mL of #1.0x10^-4 M# Sodium Chloride. Write the overall reaction. Write the net ionic equation. Will precipitate form if Ksp #AgCl# is #1.6x10^-10#?
- How do you write the Ksp expression for lead chromate (#PbCrO_4#) and calculate its solubility in mol/L? Ksp= #2.3 *10^-13#
- The Ksp for #Fe(OH)_3# = #2.5 x 10^-20#. How would you find the Ksp equation in terms of #Fe^+3# and #OH^-# concentrations?
- At 25 °C, the molar solubility of silver phosphate is #1.8 × 10^-5# mol L-1. How do you calculate Ksp for this salt?
- Silver iodide, #AgI#, has a Ksp value of #8.3 xx 10^-17#. What is the solubility of #AgI#, in mol/L?
- Barium sulfate, #BaSO_4#, is so insoluble that it can be swallowed without significant danger, even though #Ba_2^+# is toxic. At 25 °C, 1.00 L of water dissolves only 0.00245 g of #BaSO_4#. How do you calculate Ksp for #BaSO_4#?
- A saturated solution of #PbBr_2# is prepared by dissolving the solid salt in water. The concentration of #Pb_2^+# in solution is found to be 0.0115 M. What is the Ksp for #PbBr_2#?
- What is the difference between Qsp and Ksp?
- If the molar solubility of #CaF_2# at 35 C is #1.24 * 10^-3# mol/L, what is Ksp at this temperature?
- Calcium carbonate, #CaCO_3# has a Ksp value of #1.4 x 10^-8#, what is the solubility of #CaCO_3#?
- Cobalt(II) sulfide, #"CoS"#, has a #K_(sp)# value of #3.0 xx 10^(-26)#. What is the solubility of #"CoS"# in mol/L?
- A saturated solution of #Mg(OH)_2# in water has pH = 10.32. How do you calculate the Ksp of #Mg(OH)_2#?
- At a certain temperature, the solubility of barium chromate (#BaCrO_4#) is #1.8 x 10^-5# mol/L. What is the Ksp value at this temperature?
- If the #Cr_3^+# concentration in a saturation solution of #Cr(OH)_3# is #4.0xx10^-6 M#. How do you calculate the Ksp?
- What does Ksp mean in chemistry?
- What is Ksp in chemistry?
- How do you use Ksp in chemistry?
- How do you solve for Ksp chemistry?
- How do you do Ksp in chemistry?
- How does Ksp effect solubility?
- How does Ksp determine solubility?
- How does Ksp relate to solubility?
- What does Ksp in chemistry stand for?
- What is the definition of Ksp in chemistry?
- How do you use the #K_"sp"# value to calculate the molar solubility of the following compound in pure water?
- The Ksp for silver sulfate (#Ag_2SO_4#) is #1.2*10-5#. How do you calculate the solubility of silver sulfate in each of the following: a). water b). 0.10 M #AgNO_3# c). 0.43 M #K_2SO_4#?
- What is the molar solubility of #"CaF"_2# in water in terms of its #K_(sp)#?
- The solubility of lead (II) Iodate, #Pb(IO_3)_2#, is 0.76 g/L at 25*C. How do you calculate the Value of Ksp at this same temperature?
- How do you calculate Molar Solubility in grams/100mL of Calcium iodate in water at 25 degrees Celsius? Ksp = #7.1 x 10^-7#
- If 2.5mL of 0.30M #AgNO_3# is mixed with 7.5mL of 0.015M #Na_2SO_4#, should a precipitate of #Ag_2SO_4# form? (Ksp = #1.2x10^-5#)
- The concentration of #"IO"_3^(-)# ions in a pure, saturated solution of #"Ba"("IO"_3)_2# is #1.06xx10^(-3)"M"#. What is the #K_(sp)# for #"Ba"("IO"_3)_2#?
- How do we use #K_"sp"# values for solubility calculations....?
- What is the #K_(sp)# of cesium sulfate?
- How do you calculate Ksp from molar solubility?
- Question #d12fb
- Question #f4fb3
- Question #d943b
- Ksp=2.4x10^-5 for calcium sulfate. What is the molar solubility of calcium sulfate in pure water? What is the mass solubility of calcium sulfate in pure water, expressed in g/L?
- Will precipitation occur when you add 0.05 mL of 0.10 M KBr to a saturated solution of AgCl?
- Question #928c8
- Use the value ksp=1.4x10-8 for PbI2 to solve the following problems?
- Question #9f499
- What is the molar solubility of calcium sulfate in pure water?
- A salt, #AB_3#, expresses an aqueous solubility of #0.0750*mol*L^-1# with respect to the given solubility? What is #K_"sp"# for this solute?
- How do we assess solubilities of chromates, and ammonium salts?
- Question #67a25
- How do we explain the normal boiling points of #"ethanol"# (#78.4# #""^@C#), #"methanol"# (#64.7# #""^@C#), #"ethane"# (#-89# #""^@C#), #"ethyl acetate"#, (#77.1# #""^@C#), and #"methyl acetate"# (#56.9# #""^@C#)?
- Question #9e97b
- Given that #K_"sp"=1.3xx10^(-12)# for #"cuprous iodide"#, #CuI#, what mass of this salt would dissolve in a #1.2*L# volume of water?
- What is the Ksp and Kf of #Zn(H_2O)_6# ?
- Question #91010
- Question #86cf3
- Question #7445a
- What is the solubility of silver bromide in a 0.1 mol/L solution of potassium cyanide?
- Question #b226c
- Question #659e1
- What is #K_"sp"#?
- Question #0a80d
- The molar solubility of #Ag_2CO_3# is #1.3xx10^-4*mol*L^-1#. What is #K_"sp"# for this salt?
- Question #854b9
- Question #7fcb7
- Question #cb573
- Question #ae1b3
- Question #a40f4
- Question #9e5cc
- What are the molar and molal concentrations of a #9.27*g# mass of sodium chloride dissolved in #30*mL# of water?
- Question #e8dce
- What is the value of #K_(sp)# for tin(II) sulfide given that its solubility is #5.39 * 10^(−12)# #"g/100 g H"_2"O"# ?
- What is the #K_(sp)# for silver chloride?