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# Thread: Chem help, will rep for any help i can get

1. ## Chem help, will rep for any help i can get

1. If the Kb of a weak base is 7.6x10^-6, what is the pH of a 0.25M solution of this base?

2. The Ka of a monoprotic weak acid is 3.8x10^-3. What percent ionization of a 0.161 M solution of this acid?

3. Enough of a monoprotic acid is dissolved in water to produce a 0.0156 M solution. The pH of the resulting solution is 6.22. Calculate the Ka for the acid.

4. Enough of a monoprotic acid is dissolved in water to produce a 0.0134 M solution. The pH of the resulting solution is 2.63. Calculate the Ka for the acid.

5. A certain weak base has a Kb of 8.60 × 10-7. What concentration of this base will produce a pH of 10.34?

6. Using chemical equations, show how the triprotic acid H3PO4 ionizes in water. Phases, such as (l) or (aq), are optional.

7. For the diprotic weak acid H2A, Ka1 = 3.0 × 10-5 and Ka2 = 5.4 × 10-7. What is the pH of a 0.0450 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?

2. ph= [h+][oh-] 1x10^-7+1x10^-7=1X10^-14 those formulas should answer most of those.

3. bump for halp

4. Damn I used to know this stuff.

5. 6.
H3PO4 is in equilibrium with H2PO4− + H+
H2PO4− is in equilibrium with HPO42− + H+
HPO42− is in equilibrium with PO43− + H+

6. pH= -log Molarity
Ka = M^-pH

alter the equation from there to get pOH or Ka etc

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