8.00 mL of 6.00 x 10-3 MFe(NO3)3 (6.00 times 10 to the minus 3rdpower M Fe (NO3)3) is added to 8.00 mLof 8.00 x 103M KSCN (8.00 times 10 tothe minus 3rd power M KSCN) along with7.00 mL of water. The concentration of [Fe(SCN)2+] was found to be 1.00 x 10-3(1.00 times 10 to the minus 3rd power M)at equilibrium. How many initial moles ofSCN (SCN minus) are present in thesolution? Express your answer as a decimalnumber (no exponents).MYour Answer:Answerunits

We have to calculate the initial moles of SCN-.

8.00 mL of 6.00 x 10-3 M Fe(NO3)3 (6.00 times 10 to the minus 3rd power M Fe (NO3)3) is added to 8.00 mL of 8.00 x 103 M KSCN (8.00 times 10 to the minus 3rd power M KSCN) along with 7.00 mL of water. The concentration of [F e(SCN)2+] was found to be 1.00 x 10-3 M (1.00 times 10 to the minus 3rd power M) at equilibrium. How many initial moles of SCN (SCN minus) are present in the solution? Express your answer as a decimal number (no exponents). Your Answer: Answer units

8.00 mL of 6.00 x 10-3 M Fe(NO3)3 (6.00 times 10 to the minus 3rd power M Fe (NO3)3) is added to 8.00 mL of 8.00 x 103 M KSCN (8.00 times 10 to the minus 3rd power M KSCN) along with 7.00 mL of water. The concentration of [F e(SCN)2+] was found to be 1.00 x 10-3 M (1.00 times 10 to the minus 3rd power M) at equilibrium. How many initial moles of SCN (SCN minus) are present in the solution? Express your answer as a decimal number (no exponents). Your Answer: Answer units

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 115E: A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of...

See similar textbooks

Similar questions

A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?
Solid Pbl2 (Ksp = 9.8 109) is placed in a beaker of water. After a period of time, the lead(II) concentration is measured and found to be 1.1 103 M. Has the system reached equilibrium? That is, is the solution saturated? If not, will more Pbl2 dissolve?
In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?
Calculate the equilibrium concentration of Cu2+ in a solution initially with 0.050 M Cu2+ and 1.00 M NH3.
At 25C, 10.24 mg of Cr(OH)2 are dissolved in enough water to make 125 mL of solution. When equilibrium is established, the solution has a pH of 8.49. Estimate Ksp for Cr(OH)2.
The solubility of Pb(IO3)2(s) in a 7.2 102-M KIO3 solution is 6.0 109 mol/L. Calculate the Ksp value for Pb(IO3)2(s).
Calculate the molar solubility of AgBr in 0.035 M NaBr (KSP=51013).
Solutions of sodium thiosulfate are used to dissolve unexposed AgBr (Ksp = 5.0 1013) in the developing process for black-and-white film. What mass of AgBr can dissolve in 1.00 L of 0.500 M Na2S2O3? Ag+ reacts with S2O32 to form a complex ion: Ag+(aq)+2S2O32(aq)Ag(S2O3)23(aq)K=2.91013