What is the pOH of a solution obtained by adding 36.7 mL of 0.300 M NaOH...

What is the pOH of a solution obtained by adding 36.7 mL of 0.300 M NaOH (aq) to 44.3 mL of 0.200 M CH₃COOH (aq)?

Select one:

a. 2.96

b. 2.33

c. 1.58

d. 1.85

QUESTION

What is the total volume of solution at the equivalence point if a 0.100 M NaOH (aq) solution is used to titrate 15.0 mL of 0.300 M HClO₄ (aq)?

Select one:

a. 75.0 mL

b. 55.5 mL

c. 45.0 mL

d. 60.0 mL

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

What is the pH of a solution obtained by adding 50.0 mL of 0.100 M NaOH...

What is the pH of a solution obtained by adding 50.0 mL of 0.100 M NaOH (aq) to 60.0 mL of 0.100 M HCl (aq)? Select one: a. 11.96 b. 2.04 c. 3.11 d. 7.00 QUESTION 2 What is the pH of a solution prepared by dissolving 5.86 grams of propanoic acid, CH3CH2COOH (l), and 1.37 grams of NaOH (s) in enough water to make exactly 250.0 mL of solution. pKa = 4.87 for propanoic acid? Select one: a. 4.58...

A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.300 M HCl....

A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.300 M HCl. The solution was then treated with an excess of aqueous chromium(III) nitrate, resulting in formation of 2.36 g of precipitate. Determine the concentration of the solution.

2. Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH....

2. Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH. 2A. Write the net ionic equation for the reaction of phosphoric acid with NaOH to form sodium phosphate and water: 2. What is the pH of the titration medium after the addition of the following volumes of NaOH titrant: 2B. 0.00 mL : 2C. 12.50 mL: 2D. 15.00 mL: 2E. 25.00 mL: 2F. 37.50 mL: 2G: 50.00 mL 2H.60.00 mL 2I. 62.50 mL: 2J....

You prepare a diluted NaOH solution by adding 15 mL of 3 M NaOH to 435...

You prepare a diluted NaOH solution by adding 15 mL of 3 M NaOH to 435 mL of distilled water and stir for several minutes. In a clean dry beaker you obtain about 75 mL of standardized HCl and record the molarity. You take two burets, rinse one with the standardized HCl and one with the diluted NaOH solution. Fill one buret with the HCl and the other with NaOH. Prior to the titration the standard HCl soltion (~15.00 mL)...

a.) What volume (to the nearest 0.1 mL) of 4.50-M NaOH must be added to 0.300...

a.) What volume (to the nearest 0.1 mL) of 4.50-M NaOH must be added to 0.300 L of 0.150-M HNO2 to prepare a pH = 3.20 buffer? ______ mL b.) What volume (to the nearest 0.1 mL) of 4.00-M HCl must be added to 0.700 L of 0.350-M K2HPO4 to prepare a pH = 7.50 buffer? _______ mL

A titration is performed by adding 0.300 M KOH to 30.0 mL of 0.400 M HCl....

A titration is performed by adding 0.300 M KOH to 30.0 mL of 0.400 M HCl. a) Calculate the pH before addition of any KOH. b) Calculate the pH after the addition of 10.0, 25.0 and 39.5 mL of the base. c) Calculate the volume of base needed to reach the equivalence point. d) Calculate the pH at the equivalence point. e) Calculate the pH after adding 5.00 mL of KOH past the endpoint. f) Sketch the titration curve based...

A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution....

A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the addition of 20.0 mL of the HCl solution. (potentially useful info: Ka of NH4+ = 5.6 x 10−10)

a) Calculate the pH and pOH for a solution of 0.09952 M NaOH b) How many...

a) Calculate the pH and pOH for a solution of 0.09952 M NaOH b) How many acidic protons are there in 0.6137 g of KHP? c) What volume of 0.1157 M NaOH is required to obtain the endpoint of a reaction with 0.5938 g of KHP?

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of...

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCl must be added to this buffer solution to change the pH by 0.25 units? Assume the total volume remains unchanged at 400 mL. For H2PO4-, Ka = 6.3 × 10-8.

1. For a buffer solution that is made of 200.0 mL of 0.300 M HCLO with...

1. For a buffer solution that is made of 200.0 mL of 0.300 M HCLO with 100.0 mL of 0.200 M KCLO. The Ka for HCLO is 2.9*10^8. What is the PH of the buffer? 2. Consider the same solution. To this solution, if 10.00 mL of 0.100 M HCl is added, what is the new pH? *both answers to 2 decimal places*

Subjects