It is found that up to 0.0980 g of AgIO3 dissolves in 2.00L of aqueous solution at a certain temperature. Determine the value of Ksp for AglOs. PREV Based on the set up of your ICE table, construct the expression for Ksp and then evaluate it. Do not combine or simplify terms. Ksp [1.73 x 101 [1.73 × 10 2.99 x 10-8 %3D 5 RESET [0] [0.0980] [0.0490] [1.73 x 10-] [3.47 х 10-] [1.73 х 10 ] [0.0980]? [0.0490]? [1.73 х 10-P [3.47 x 10 [1.73 х 10-p [x] [2xP [3.47 х 104 + х]| [3.47 х 104-х] [1.73 x 10 + 2x] [1.73 x 10* - 2x] 1.20 х 107 2.99 х 10в 6.00 х 10в

The molar solubility of lead(II) iodate at 25 °C is 40.0 μmol L-1 . Calculate the value ofthe solubility product Ksp for lead(II) iodate

Given that Ka for HIO is 3.2 × 10-1" at 25 °C, what is the value of K, for IO¯ at 25 °C? Kp = Given that Kp for CH, NH, is 5.0 x 10-4 at 25 °C, what is the value of Ka for CH, NH; at 25 °C? Ka =

Consider a reaction with a large negative Gibbs energy change, as shown below: 42.6 kJ mol-1 Y Z , AG°/ = The reaction is initiated by adding 16 mmol of compound Y into the flask, in the absence of compound Z is present. After 48 hours, analysis reveals the presence of 4 mmol of Z and 12 mmol of Y. Which is the most likely explanation? ▪▪▪▪▪▪ - OY and Z have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward Y. Formation of Z is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Z is thermodynamically unfavorable. Two of the above explanations are reasonable.