Solubility Rules applied to various reactions
Use the Solubility Rules to write net ionic equations for the reactions that occur when solutions of the following are mixed. a) K2S + ZnSO4 b) K2CrO4 + NiCl2 c) CsOH + FeCl3 [2] d) CuSO4 + Pb(ClO4)2 e) FeSO4 + K3PO4 f) FeCl2 + TlNO3 g) (NH4)2CO3 + Ni(ClO4)2
Please show how to solve. Calculate the pH of CO2-saturated water at 25 degrees C, given that the CO2 concentration in air is 338 and that for carbon dioxide the Henry's Law constant KH=3.4E-2 mol L-1 atm-1 at 25 degrees C. Furthermore, the ionization constant, Ka, for H2CO3 has a value of 4.5E-7 mol L-1 at this temperature. ...continues
I have looked at a solution and was not able to come up with a correct answer. Please show how to solve this problem: What is the calculated value of the partial pressure(atm) of O2 in acid mine water of pH 2.700, in which [Fe3+] = [Fe2+]? Hint: Application of the Nernst Equation
I have already looked at a few solutions and none have worked to come up with a correct solution. Please show how to solve this problem. A ground water sample , at 25 C, has Eh= 1.0 and pH=6.80. Assuming the system is at equilibrium, calculate the amount of dissolved oxygen (ppm) in the groundwater sample.
I thought I had the answer but I was wrong. Please show how to solve. Calculate the mass percent of methanol, ethanol, and MTBE each that must be present in gasoline to yield a mixture of 2.9 % oxygen by weight. Hint given: Calculate percent oxygen in each compound. I don't have the density of the gasoline in the ques ...continues
Weak acid and corresponding ion concentrations.
What are pH, [H3O+], [HSO3–], and [SO32–] in a 1.50 M sulfurous acid solution?
If the concentration of atmospheric CO2 were to double from its current value of 390 ppm, what would be the calculated pH of rainwater assuming that CO2 was the only acidic input?
