Chemistry, 26.10.2021 08:00, mjweed3381
Equilibria can be treated mathematically with the equilibrium constant, K. For the reaction Fe^3+ + SCN β equilibrium reaction arrow FeSCN^2+, the equilibrium constant expression is [FeSCN^2+β] K = [Fe^3+β] Β· [SCN ββ] where, for example, [Fe3+β] is the molar concentration (mol Fe^3+ / L solution) present in an equilibrium mixture. At some temperature, a chemist found the following equilibrium concentrations. [Fe3+β] = 8.17βββ10^β3 M, [SCN ββ] = 8.60βββ10^β3 M, [FeSCN^2+β] = 6.25βββ10^β2 M
a. What is value of K?
Suppose that some FeSCN^2+ is added to the above solution to shift the equilibrium. When equilibrium is re-established, the following concentrations are found.
[Fe3+β] = 8.34βββ10^β3 M, [SCNββ] = 8.77βββ10^β3 M
b. What is the concentration of FeSCN2+ in the new equilibrium mixture?
Answers: 3
Chemistry, 22.06.2019 22:40, lindseyklewis1p56uvi
Percent ionization for a weak acid (ha) is determined by the following formula: percent ionization=[ha] ionized[ha] initialΓ100%for strong acids, ionization is nearly complete (100%) at most concentrations. however, for weak acids, the percent ionization changes significantly with concentration. the more diluted the acid is, the greater percent ionization. a certain weak acid, ha, has a ka value of 9.4Γ10? 7.part acalculate the percent ionization of ha in a 0.10 m solution. part bcalculate the percent ionization of ha in a 0.010 m solution
Answers: 1
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