Determine the pH change when 0.093 mol HI is added to 1.00 L of a buffer solution that is 0.397 M in HNO2 and 0.365 M in NO2-.

A 0.2649-g sample of a monoprotic acid neutralizes 53.8 mL of 0.07193 M KOH solution. Calculate the molar mass of the acid. 4.0 | g/mol

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?

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