You are directed to prepare 100 mL of a 500 mEq/L KOH standard. The primary standard used has a concentration of 0.400 Eq/L. When titrating your KOH solution, you discover that 4.0 mL of the primary standard reacted exactly with 5.0 mL of the KOH solution. a. What is the actual Eq/L concentration of the KOH solution? b. How many mEq are required to adjust the volume and concentration of the remaining 85 mL of KOH solution to 100 mL of a 500 mEq/L KOH solution? c. How many mL of 12 Eq/L KOH stock must be added in order to adjust the concentration of the KOH standard to 500 mEq/L?

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] =

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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?

You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity   Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?

In the titration of 25.00 mL of a water sample, it took 19.040 mL of 4.965x 10−3 M EDTA solution to reach the endpoint.   Convert the number of mL of bottled water used in each sample titration to Liters. (enter your answer with 3 significant figures)

Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g

8. A student conducts an acid-base titration to investigate the change in pH during a reaction between hydrochloric acid and ammonia solution. a. Name a piece of equipment that could be used to provide an accurate measurement of pH during the titration and explain how it would be calibrated. The student transfers 50cm3 of 1.0moldm3 ammonia solution acid into a beaker. During the titration the student adds 50cm3 1.00moldm³ hydrochloric acid from a burette into the beaker and records the pH throughout. b. Sketch the pH curve produced during this titration.

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

2. A buffer solution is prepared by mixing 15.00 mL of 0.12 M CH COOH with 9.00 mL of 0.080 M NaOH. a. Calculate the moles of CH COOH and NaOH before mixing. b. Assuming the reaction goes to completion, calculate the moles of CH₂COOH and CH COO present in the buffer solution. c. Calculate the concentration of CH COOH and CH COO in the buffer solution. d. Use the Henderson-Hasselbalch equation to calculate the expected pH of this buffer solution. CH COOH K₂ = 1.8 x 10.