Calculate the molar solubility of copper(II) sulfide in each liquid or solution.
A) pure water
B) 0.27 M CuCl2
C) 0.23 M K2S
We need to have access to the solubility product [Ksp] value of the CuS to solve this question. Using the value of solubility product as 6 * 10-37 we will be solving the question.
In the second and the third part of the question we will be using the common ion effect.
Common in Effect - In presence of common ion in the solution coming from some other salt, the solubility of Cus will decrease. The concentration of common ion will remain same throughout the solution. In the common ion effect the molar solubility of the uncommon ion is taken as the molar solubility of Cus.
Calculate the molar solubility of copper(II) sulfide in each liquid or solution. A) pure water B)...
The molar solubility of copper(II) carbonate in a water solution is____ M. Ksp= 2.5x10^-10 The equilibrium concentration of zinc ion in a saturated zinc sulfide solution is _____ M. Ksp= 2.0x10^-25
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)...
A student measures the molar solubility of iron(II) sulfide in a water solution to be 2.14×10-9 M. Based on her data, the solubility product constant for this compound is_____
will the ange 107 45. Calculate the molar solubility of barium fluoride in each liquid or solution. a. pure water b. 0.10 M Ba(NO3)2 c. 0.15 M NaF orm
will the ange 107 45. Calculate the molar solubility of barium fluoride in each liquid or solution. a. pure water b. 0.10 M Ba(NO3)2 c. 0.15 M NaF orm
A student measures the molar solubility of copper(II) carbonate in a water solution to be 1.53×10-5 M. Based on her data, the solubility product constant for this compound is ?
The molar solubility of copper(II) carbonate in a 0.133 M copper(II) acetate solution is M.
Calculate the molar solubility of lead thiocyanate in pure water. The molar solubility is the maximum amount of lead thiocyanate the solution can hold. Lead thiocyanate has a Ksp value of 2.0*10^-5.
please someone help me with these questions.. thanks so
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The molar solubility of copper(II) carbonate in a 0.277 M sodium carbonate solution is Submit Answer Retry Entire Group 4 more group attempts remaining The molar solubility of copper(II) sulfide in a 0.237 M copper(II) nitrate solution is Submit Answer Retry Entire Group 4 more group attempts remaining Use the References to access important values if needed for this question The concentration of iron(II)ion Solid iron(II) nitrate is slowly added...
1) Using Appendix D, calculate the molar solubility of AgBr in (a) pure water, (b) 3.0x10-2 M AgNO3 solution, c) 0.10 M NaBr solution. 2) Calculate the solubility of Mn (OH)2 in grams per liter when buffered at pH (a) 7.0, (b) 9.5, (c) 11.8