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- The pH for 0.050 M CH3NH2 (Kb for CH3NH2 = 4.0 X 10^-4 )?What is the pH of the solution after mixing 0.171 g of Mg(OH)2 (MW=58.321 g/mol) with 68.9 mL of 0.0569 M HCl? The resulting solution was diluted to 100 mL. Round your calculated value for pH to two figures to the right of the decimal point.You start with a 10.0 mM solution of H3PO4 at a pH of 7.0. If you were to add 2.0 mL of 100 mM HCl what would the resulting pH be? Please show work.
- Kb for methylamine at 25°C is 4.4 x 10-4 what is its pH if 0.10M solution is used.When calculating the PH for a .023 mole solution of HBrO2. My Ki is 2.1x10-4 and PH is 2.6. However Calculate the PH for a solution that is .023 M in HBrO2 and .03M in Ca(BrO2)2? Ki for HBrO2 = 2.1x10-4 Will that increase my PH?Hello, can someone please help me with these chem questions and give me a clear step-by-step solution. Thank you very much for your help. a)The [H3O+], in M, of 10.00 mL of 0.100 M NaOH after adding 10.00 mL of indicator solution. To enter exponential values, use the format 1.0e-5. b)The [H3O+], in M, of 10.00 mL of 0.100 M HCl after adding 10.00 mL of the indicator solution. To enter exponential values, use the format 1.0e-5.
- Calculate the pH of a weak acid which dissociates as AH ⇌ A- + H+ ( like CH3COOH ⇌ CH3COO- + H+ or HNO2 ⇌ NO2- + H+ ) knowing that the initial concentrations are [AH]0 0.11 M and the acid dissociation constant, Ka , is 5.86e-7 pH _______ ← please insert your valueThe value for Kw at 0.0°C is 1.14 x 10^-15. Calculate the pH for a neutral solution at this temperature.What is the pH of a solution that has a [OH-] of 8.5 x 10-4 please show work
- v. What is pH? Calculate the pH for 0.0001N NH4OH solution of 100mL volume. The pKb value for NH4OH at 25oC is 1.76 x 10-5.calculate the PH of 1.5 M solution of hydroxylamine at 25 degrees C with a Kb = 9.1 times 10^-9Can you please answer A-C and show all of the steps to the solution please and thank you