Question

Below is the result of a student's efforts to determine the solubility product, Ksp, of strontium chromate. The concentration of Sr2+ in the reference cell is 0.00100 M. The concentration of chromate in the nonreference cell was calculated to be 0.993 M. The voltage of this nonreference cell relative to the reference was measured as -49.0 mv. The temperature is 25.0 C NOTE The voltage is recorded as negative due to the way the silver electrodes are placed in the reference and nonreference half-cells. Real cell voltages are always POSITIVE. So, change your voltage to POSITIVE VOLTS, plug all your values into the Nerst Equation, and solve for the concentration of (M) of the Sr2+ in equilibrium with the precipitate and chromate in the nonreference cell nonref] [nonref ] [ ref] 2.303 RT log - 4503 RT n 96,500 + V_ 2.303 Enter your answer to the correct number of significant figures. Do not include units with your answer. Enter Your Answer: Use the concentration of chromate given in Question 3, your answer to Question 3 and Equation 6.2 to calculate the solubility product, Ksp, of strontium chromate. Enter a numeric answer to the correct number of significant figures. Enter Your Answer:

Answer 1

ce cell 0.001 M n No. eledvon involve d2 This is on Apoinat Moluble salt 9550 TReb 8:214 X 298 96500 2 303 2.214 x 298 x 2, 996 ー-2-3o3 V .. o , o 8 860 volt bul Polenlial Positlive in) V 0.0 886 Vold 0.999广 P 098