What mass of sodium formate must be added to 550.0 mL of 1.30 M formic acid to produce a buffer solution that has a pH of 3.40 (Ka [HCOOH]) =1.80 x 10 ^-4)?
What mass of sodium formate must be added to 550.0 mL of 1.30 M formic acid...
What volume, in mL, of 2.00 M HCl must be added to 1.00 L of a 0.100 M solution of sodium formate, Na+HCOO-, to produce a buffer solution having a pH = 4.00? (Ka HCOOH = 1.9 x 10-4) A. 17 B. 1.9 C. 34 D. 30 E. 3.5
Answer Part B please 1.000 mol of formic acid (HCOOH) and 0.500 mol of sodium formate (NaCOOH) are added to water and diluted to 1.00 L. Calculate the pH of the solution. Ka 1.77 x 10-4 (4 marks) Enough HCl is added to the above solution (with negligible volume change) to bring the [H3O] up to 0.100 M. Find the pH of the resulting solution. (5 marks)
how many grams of sodium formate must be dissolved in a 0.300 M solution of formic acid to make 400.0 ml of a buffer solution with a pH=4.60?
inn? 1. Formic acid, (K= 1.8x10) a WA, and sodium formate, its' CB, are mixed together in a 250.0 mL volume of 0.350 M formic acid and 0.455 M sodium formate- to form a buffer solution. a. If 1.00 mL of 1.00 M HCI is added to 250.0 mL of DI water, what is the new pH? What is the pH if the 250.0 mL of solution was only 0.350 M HCOH (no formate)? b. c. What is the pH...
3. (5 pts) Find mass of sodium formate to be added to 25.0 mL of 0.25 M solution of formic acid so that after dilution to 100.0 mL the resulting solution has pH = 4.0. The acid dissociation constant of formic acid is 1.8x10".
4. Briefly explain the meaning of the term buffer capacity". A formic acid/sodium formate solution would be expected to buffer around what pH (use your textbook)? a) Calculate the pH for a solution containing 3.48 M CSHSN and 2.52 M C H NHBr. (Kb - 1.40 x 10" for CsH:N) Calculate the pH after 150.0 mL of 3.16 M HCl is added to 875.0 mL of the solution in part a) above.
4. Formic acid, HFor, has a Ka value of 1.8 × 10 -4 . A student is asked to prepare a buffer having a pH of 3.40 from a solution of formic acid and a solution of sodium formate having the same molarity. How many milliliters of the NaFor solution should she add to 20 mL of the HFor solution to make the buffer? 5. How many mL of 0.10 M NaOH should the student add to 20 mL 0.10...
Calculate the pH of a solution made by adding 48.0 g of sodium formate, NaHCOO, to 100. mL of 0.21 M formic acid, HCOOH. Hint what kind of solution is made? The Ka for HCOOH is 1.8 x 10-4 M. As usual, report pH to 2 decimal places.
Calculate the pH of a solution made by adding 34.0 g of sodium formate, NaHCOO, to 400. mL of 0.31 M formic acid, HCOOH. Hint what kind of solution is made? The Ka for HCOOH is 1.8 x 10-4 M. As usual, report pH to 2 decimal places.
2. A Student wants to prepare 250.0 mL of pH 4.1 buffer solution. He is planning to use formic acid (HCOOH) and sodium formate (HCOONa) for this job. What should the mass of sodium formate that he should add to 250,0 mL of 0.20 M formic acid solution to prepare this buffer? (K =1.8x10 for formic acid.) 3. If 0.10 M solution of a weak acid has a pH of 3.90, find the Ka for the acid.