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Question 3 3 pts 3. A 2.5 M HCl solution is used to titrate (neutralize) a...
Question 38 2.5 pts Suppose 19.2 mL of 0.489 M HCl was used to titrate an unknown sample of KOH (molar mass 56.11 g/mol). What mass of KOH was in the sample? The balanced chemical equation is: HCI + NaOH- NaCl + H20 O 0.114g O 0.527 g O 0.437 g 0 3.42 g
A 0.205 M NaOH solution is used to titrate 20.0 mL of solution of H2SO4. Write a balanced equation for this acid base reaction If 45.6 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4solution. What is the PH of the solution if the hydroxide concentration [OH-] is 4.3 x 10-6M.
29 ml of .09693 M HCl is used to neutralize a 0.2289 g sample of an unknown base. The pH of the final titrated solution was 4.13. What is the pKa of the conjugate acid of the base?
1. How many mL of 0.100 M NaOH are required to neutralize (or titrate) 25.0 mL of 0.15 M H,Po.? Write the balanced acid-base neutralization reaction to start. (12 pts)
An aqueous solution of Ca(OH)2with a concentration of 0.143 M was used to titrate 25.00 mL of aqueous HCl. 14.73 mL of the Ca(OH)2was required to reach the endpoint of the titration. How many moles of base were required to react completely with the acid in this reaction? How many moles of HCl were present in the original 25.00 mL of acid? What is the molarity of the original HCl solution? 04 Question (a points) aSee page 166 Watch the...
what volume of 2.5 NaOH is needed to neutralize a 135 ml of 1.15 M HCL solution?
i need help with understanding 7a,7b, and 7c A 2 M NaOH is used to titrate 1000 mL of a solution of HCI (hydrochloric acid), the concentration of which is unknown. If 100 mL of 2 M NaOH is required to neutralize the HCI solution: 7. How many moles of NaOH were added? How many moles of HCI were present in the unknown solution? What was the concentration of the unknown solution of HCI?
2. In an acid-base titration, 25.62 mL of an NaOH solution are needed to neutralize 26.23 mL of a 0.1036 M HCI solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of M in the HCl solution. a. H* b. Find M Oн in the NAOH solution. (Use Eq.3.) from MOH NaOH c. Obtain M.
You titrate 25.0 mL of 0.100 M HCl solution with 0.086 M NaOH. What is the limiting reactant?You titrate 25.0 mL of 0.100 M HCl solution with 0.086 M NaOH. What is the final [H3O+]?You titrate 25.0 mL of 0.100 M HCl solution with 0.086 M NaOH. What is the final pH of the solution?
0.85 mL of 2.4 M NaOH was added to neutralize 45.0 mL of a H3PO4 solution. a) write the balanced molecular equation b) calculate the concentration of the phosphoric acid solution 6. 0.85 mL of 2.4 M NaOH was added to neutralize 45.0 mL of a H3PO4 solution. (10 points) a) Write the balanced molecular equation. b) Calculate the concentration of the phosphoric acid solution.