1. A student performs a titration that requires 40.00 mL of 0.5000 M KOH to completely...

Question

Question

science chemistry

Answer 1

Answer #1

Date: According تلحلل land) (Base) N = nom L, no factor baraty No of equals to acidity oxidation statel electione exchanged -

Answer 2

Similar Homework Help Questions

If a 25.0 mL sample of phosphoric acid, H3PO4, is completely neutralized by 137 mL of...

If a 25.0 mL sample of phosphoric acid, H3PO4, is completely neutralized by 137 mL of 0.100 M KOH, what is the molarity of the phosphoric acid? Given: H3PO4 + 3 KOH → 3 H2O + K3PO4
In a titration, a student found that 42.6 mL of a KOH solution were required to...

In a titration, a student found that 42.6 mL of a KOH solution were required to neurtralize 28.9 mL of a 0.160 M sulfuric acid solution. Determine the molarity of the KOH solution. SHOW WORK. 2KOH(aq) + H2SO4(aq) ------> K2SO4(aq) + 2H2O(l)
2. A student performs a titration on a 5.00 mL sample of an HBr solution. She...

2. A student performs a titration on a 5.00 mL sample of an HBr solution. She uses 24.32 mL of a 0.459 M KOH solution to reach a phenolphthalein endpoint. (See Example 2, if necessary.) a. Write the balanced equation for the reaction. Remember to include the correct physical states for each reactant and product in your balanced equation. b. How many moles of KOH were used? C. How many moles of HBr were present? d. What is the molarity...

An unknown concentration of phosphoric acid is titrated to its equivalence point with 0.2701 M KOH....

An unknown concentration of phosphoric acid is titrated to its equivalence point with 0.2701 M KOH. What is the concentration of the acid? H3PO4 (aq) + 3 KOH(aq) - K3PO4 (aq) + 3 H2O) Initial volume of KOH solution 1.03 mL Final volume of KOH solution 15.02 mL Original volume of H3PO4 solution 24.68 mL O 0.001260M 0.05104 M 0.1531 M 0.4593M
H3PO4(aq) + 3 KOH(aq) → K3PO4(aq) + 3 H2O(l). You mix 750. mL of 0.1250 M...

H3PO4(aq) + 3 KOH(aq) → K3PO4(aq) + 3 H2O(l). You mix 750. mL of 0.1250 M H3PO4 with 750. mL of 0.350 M KOH What is the theoretical yield of water produced - in grams?
25.00 mL of HCl (aq) solution requires 18.92 mL of 0.1024 M NaOH to react completely...

25.00 mL of HCl (aq) solution requires 18.92 mL of 0.1024 M NaOH to react completely in an acid-based neutralization reaction. What is the molarity of the HCl solution?

If 38.2 mL of 0.159 M KOH is required to neutralize completely 27.0 mL H2SO4 solution,...

If 38.2 mL of 0.159 M KOH is required to neutralize completely 27.0 mL H2SO4 solution, what is the molarity of the acid solution? H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l)
If 35.2 mL of 0.171 M KOH is required to neutralize completely 26.0 mL H2SO4 solution,...

If 35.2 mL of 0.171 M KOH is required to neutralize completely 26.0 mL H2SO4 solution, what is the molarity of the acid solution? H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l)
A. Titration of a 11.0 mL solution of KOH requires 12.0 mL of 0.0310 M H2SO4...

A. Titration of a 11.0 mL solution of KOH requires 12.0 mL of 0.0310 M H2SO4 solution. B. If 28.0 mL of a 0.200 N acid solution is needed to reach the end point in titration of 17.5 mL of a base solution, what is the normality of the base solution?

1. How many milliliters of 0.112 M Na2CO3 will completely react with 27.2 mL of 0.135...

1. How many milliliters of 0.112 M Na2CO3 will completely react with 27.2 mL of 0.135 M HNO3 according to the reaction 2HNO3(aq) + Na2CO3(aq) → H2O(l) + CO2(g) + 2NaNO3(aq) Part B.) A 25.0-mL sample of HNO3 solution requires 35.7 mL of 0.108 M Na2CO3 to completely react with all of the HNO3 in the solution. What is the concentration of theHNO3 solution? Part C.)Consider the reaction HCl(aq) + NaOH(aq) → NaOH(aq) + H2O(l) How much 0.113 M NaOH...