For 280.0 mL of a buffer solution that is 0.240 M in HCHO2 and 0.315 M in KCHO2KCHO2, calculate the initial pH and the final pH after adding 0.024 mol of NaOH. ( Ka(HCHO2)=1.8×10−4)

Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸. Determine the moles of the ractant and product after the reaction of the acid and base. (Similar to ICE format but is instead Before (mol), Change (mol), and After (mol) Determine the ICE table for HClO (aq) + H2O - H3O+ + ClO- (aq) Fill in Ka= ? = 2.9 * 10-8 Calculate pH

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?

What is the [H3O+] and the pH of a buffer that consists of 0.29 M HNO2 and 0.77 M KNO2? (Ka of HNO2 = 7.1 * 10−4)

Use the References to access important values if needed for this question. A buffer solution is made that is 0.379 M in HCN and 0.379 M in NaCN. If Ka for HCN is 4.00 x 10-¹0, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.090 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + Submit Answer ->> Retry Entire Group + 9 more group attempts remaining

do both please as they are the part of the same question..

We have 500.0 mL of a buffer solution that is 0.697 M in NH3 and 0.380 M in NH4Cl. We add 500.0 mL of a solution 0.202 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?

For 480.0 mL of a buffer solution that is 0.160 M in CH3CH2NH2 and 9.00×10−2 M in CH3CH2NH3Cl , calculate the initial pH and the final pH after adding 1.5×10−2 mol of HCl . ( Kb(CH3CH2NH2)=5.6×10−4 .)

Calculate the initial pH and the final pH after adding 0.0150 mol of NaOH. For 230.0 mL of a buffer solution that is 0.2604 M in CH3CH2NH2 and 0.2404 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.0150 mol of NaOH(Kb=5.6⋅10^−4).

Calculate the pH of a buffer solution that is 0.200 M in HCN and 0.120 M in NaCN.  The Ka of HCN is 4.90 x 10-10.