You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC HO, abated KHP) as the primary standard. KHP (molar mass = 204.22 ganol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 50.75 mL of HCI solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCI solution?

5 b) Benzoic acid, HC7H5O2, is a weak monoprotic acid. A stock HC,H5O2 solution with unknown concentration was prepared. A 25.00 mL sample of the stock HCH5O2 solution was titrated with 0.1234 M sodium hydroxide to the equivalence point, using phenolphthalein as an indicator. The titration took 20.26 mL of titrant (sodium hydroxide). (b) Write a balanced complete ionic equation for the chemical reaction that occurs in this titration.

15.00 mL of 0.214 M oxalic acid, H2C2O4 ,solution was placed in an Erlenmeyer flask.  0.237 M KOH  solution was used to titrate the solution in the flask.   H2C2O4 is a diprotic acid and the Hs that are shown in blue are the Hs that will react with the hydroxide ion of a base. During the titration, KOH solution was added until ________ moles of H2C2O4 were in the reaction flask.

Part B The titration of 0.5538 g of KHP required 25.89 mL of an NaOH solution to reach the equivalence point. What is the concentration of the NaOH solution? Express your answer using four significant figures. ΑΣΦ M NaOH] =

The formula H₂SO4 + 2 KOH --> K₂SO4 + 2 H₂O describes the reaction between sulfuric acid and potassium hydroxide. In the titration done, 20 mL of KOH with an unknown concentration is put into a flask with bromthymol blue indicator. The KOH solution was titrated with a 0.25 M H₂SO4 solution. Three trials were performed and each trial yielded to an endpoint of yellow-colored solution, which is the desired endpoint. After three trials, the following readings were obtained: 15.5, 15.1, and 14.9 mL respectively. Calculate the molarity of Potassium hydroxide. (Answer must be rounded off to 2 decimal places)

An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution?   2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution?   3. What is the concentration of Ag+ in solution?

Question 25 of 30 Submit You prepare a standard NAOH solution for the laboratory, using potassium hydrogen phthalate (KHC§H,0a, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/ mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC6H,O6, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 19.74 mL of the NaOH to titrate (react exactly with) | % 1 4 6. C 7 +/- x 10 0 Tap here or pull up for additional resources LO 00

A 2.2004 g of primary standard oxalic acid, H2C2O4 (90.04 g/mol), was dissolved in water to form a 250.00 mL solution. A 50.00 mL aliquot was taken for analysis and required 51.62 mL NaOH for titration. If the reaction is: H2C2O4 + 2NaOH ----> Na2C2O4 + 2H2O, what is the molarity of the NaOH solution?

7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation.           H3C6H5O7  (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?

What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Present complete solutions for the following problem. Express your final answers up to two (2) decimal places.