You standardize your NaOH solution by titrating a known quantity of sulfamic acid (H2NSO3H) standard. It requires 36 mL of the solution to reach the endpoint with 0.2913 g of sulfamic acid. What is the concentration of your NaOH solution?
I got 0.08333, but it is wrong.
You standardize your NaOH solution by titrating a known quantity of sulfamic acid (H2NSO3H) standard. It...
Potassium hydrogen phthalate, abbreviated KHP, is used to standardize NaOH solutions. A standard KHP solution is made by dissolving 2.12 grams of KHP in 100.00 mL of water. The KHP solution is then titrated with NaOH solution. It takes 23.12 mL of NaOH to reach the endpoint. What is the concentration of the NaOH?
A titration to standardize a NaOH titrant by titrating it against the monoprotic primary standard base “TRIS” is performed in lab, with the following data being gathered: Titration of 25.00 ± 0.03 mL TRIS solution (0.1102± 0.0004 mol/L) Initial buret reading: 0.42 ± 0.01 mL Final buret reading: 15.77 ± 0.01 mL The concentration of the NaOH titrant is: ( ) ± ( ) mol/L.
Part A You are given a solution of HCOOH (formic acid) with an approximate concentration of 0.20 M and you will titrate this with a 0.1105 M NaOH. If you add 20.00 mL of HCOOH to the beaker before titrating, approximately what volume of NaOH will be required to reach the end point? You are given a solution of (formic acid) with an approximate concentration of 0.20 and you will titrate this with a 0.1105 . If you add 20.00 of to the beaker before...
As part of Lab 11 you will make and standardize a solution of NaOH(aq). Suppose in the lab you measure the solid NaOH and dissolve it into 100.0 mL of water. You then measure 0.1993 g of KHP (204.22 g/mol) and place it in a clean, dry 100-mL beaker, and then dissolve the KHP in about 25 mL of water and add a couple of drops of phenolphthalein indicator. You titrate this with your NaOH(aq) solution and find that the...
If 0.654 g of a primary standard acid (potassium hydrogen phthalate, molar mass = 204.23 g/mol) requires 24.42 mL of a NaOH solution of unknown concentration to reach an endpoint. What is the concentration of NaOH?
answer (2)
2. Suppose that you used a known concentration (0.8442 M) of Ca(OH)2 to determine the concentration of an unknown HBr solution. If it takes 12.88 mL of the Ca(OH)2 solution to titrate 15.00 mL of the unknown HBr solution, what is the molarity of the HBr? 1. A solid diprotic weak acid, H2A (molecular weight = 128.9 g/mol) is used to standardize a KOH solution. When 0.4228 g of the acid is dissolved in 40.0 mL of water...
Question 4 Status: Not yet answered | Points possible: 1.00 Suppose you are titrating an acid of unknown concentration with a standardized base. At the beginning of the titration, you read the base titrant volume as 2.86 mL. After running the titration and reaching the endpoint, you read the base titrant volume as 21.17 mL. What volume, in mL, of base was required for the titration? Type answer: Question 6 Status: Not yet answered Points possible: 1.00 Suppose you are...
You are titrating a weak acid and after 40.0 mL of NaOH solution is added, the pH =4.00. After 60.0 mL more of the NaOH is added, the titration indicator turns color. What is the Ka of this acid ?
A student is asked to standardize a solution of barium hydroxide. He weighs out 0.912 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid). It requires 15.2 mL of barium hydroxide to reach the endpoint. A. What is the molarity of the barium hydroxide solution? M This barium hydroxide solution is then used to titrate an unknown solution of perchloric acid. B. If 12.6 mL of the barium hydroxide solution is required to neutralize 27.7 mL of perchloric acid,...
A student is asked to standardize a solution of potassium hydroxide. He weighs out 0.911 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid). It requires 31.0 mL of potassium hydroxide to reach the endpoint. A. What is the molarity of the potassium hydroxide solution? M This potassium hydroxide solution is then used to titrate an unknown solution of hydrobromic acid. B. If 25.2 mL of the potassium hydroxide solution is required to neutralize 27.6 mL of hydrobromic acid,...