Calculate the pH of the following solution: 50.00 mL of 0.09271 M NaOH [OH-] of this solution = 0.09271 M Next step is to calculate the concentration of H+ ions from [OH-] using Kw.
[H+]= ? M
Calculate the pH of the following solution: 50.00 mL of 0.09271 M NaOH [OH-] of this...
Calculate the pH of a mixture of 51.0 mL of 0.106 M NaOH and 50.00 mL of 0.0950 M HNO3.
Calculate the pH of a solution formed by mixing 50.00 mL of 0.0100 M HNO3 with 30.00 mL of 0.0150 M solution of Ba(OH)2
Calculate [OH -] and pH for each of the following solutions. (a) 0.0010 M NaOH [OH-] = M pH = (b) 0.0267 g of LiOH in 550.0 mL of solution [OH -] = M pH = (c) 69.4 mL of 0.00138 M Sr(OH)2 diluted to 600 mL [OH -] = M pH = (d) A solution formed by mixing 49.0 mL of 0.000590 M Sr(OH)2 with 77.0 mL of 4.2 x 10-3 M NaOH [OH -] = M pH =
Calculate [OH -] and pH for each of the following solutions. (a) 0.0013 M NaOH [OH-] = ____M pH =_____ (b) 0.0571 g of CsOH in 540.0 mL of solution [OH -] ____= M pH =____ (c) 11.6 mL of 0.00247 M Ba(OH)2 diluted to 800 mL [OH -] = ___ M pH =___ (d) A solution formed by mixing 82.0 mL of 0.000500 M Ba(OH)2 with 54.0 mL of 6.4 x 10-3 M NaOH [OH -] = ___M pH...
A 50.00 ml aliquot of 0.1000 M NaOH is titrated with 0.1000 M HCL. Calculate the pH of the solution after the addition of 0.00, 10.00, 25.00, 40.00, 45.00, 49.00, 50.00, 51.00, 55.00, and 60.00 ml of acid and prepare a titration curve from the data.
Calculate the pH of a mixture when 48.00 mL of 0.100 M NaOH solution is added to 50.00 mL of 0.100 M HCl solution? Write the correct answer in 3 significant figures.
1) Calculate the pH in the titration of 50.00 mL of 0.060 M acetic acid (CH3COOH) with a 0.120 M sodium hydroxide, NaOH solution after the addition of the following volumes of base: Ka for acetic acid = 1.8 x 10-5 A) 0 mL pH = B) 10 ml pH =
Titrations 1. A 50.00-ml NaOH sample of unknown concentration was titrated with 0.1274 M HCI. if 33.61 mL of the HCl solution were required to neutralize the NaOH sample, what is the molarity of the NaOH sample? Show the steps in your calculation 2. A 25.00-ml HCl sample of unknown concentration was titrated with 0.5631 M Al(OH)3. If 37.62 mL of the Al(OH) solution were required to neutralize the HCl sample, what is the molarity of the HCl sample? (Assume Al(OH)3 is...
4. (36 pts) Calculate the pH after the addition of 15.00, 25.00, 40.00, and 50.00 mL of 0.400 M NaOH to a solution that contains 100.00 mL of 0.100 M HIO HIO (a)+H20U) »HI(aq)+H, (aq) H 10% (a) H,O)H I0%(a)HO(aq) K, = 2.0 x 10-2 -9 k,-5.0 × 10 a2 4. (36 pts) Calculate the pH after the addition of 15.00, 25.00, 40.00, and 50.00 mL of 0.400 M NaOH to a solution that contains 100.00 mL of 0.100 M...
a) 28.3 mL of a 0.200 M NaOH solution is required to titrate a 200.0 mL sample containing HCl to its equivalence point. What was the concentration of HCl in the solution with which you started? b)The pH of blood is = 7.4. What is the concentration of OH- ions?