A 0.205 M NaOH solution is used to titrate 20.0 mL of solution of H2SO4. Write...
- 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.
Homework Answers
first write the balanced equation and then by using the
dilution law find the molarity of H2SO4 as follows
Add Answer to:
A 0.205 M NaOH solution is used to titrate 20.0 mL of solution
of H2SO4.
Write...
7) Titrate 20.0 mL of HNO3 with an unknown concentration with 15.4 mL of 0.300M NaOH....
7) Titrate 20.0 mL of HNO3 with an unknown concentration with 15.4 mL of 0.300M NaOH. Determine HNO3 concentration. Neutralization equation of nitric acid (HNO3) with NaOH is: HNO3 + NaOH + H2O + NaNO3 8) Titrate 25.00 mL of Ca(OH)2 solution with unknown concentration with 15.65 mL of 1.50M H3PO4. Determine the Ca(OH)2 concentration. Neutralization equation of phosphoric acid with calcium hydroxide is: H3PO4 + Ca(OH)2 + H2O + Ca3(PO4)2 (unbalanced)
An aqueous solution of Ca(OH)2with a concentration of 0.143 M was used to titrate 25.00 mL...
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...
A solution of 0.154 M NaOH is used to neutralize 25.5 mL of a H2SO4 solution....
A solution of 0.154 M NaOH is used to neutralize 25.5 mL of a H2SO4 solution. If 25.0 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4 solution? H2SO4(aq)+2NaOH(aq)→2H2O(l)+Na2SO4(aq)
A 0.080 M NaOH solution was used to titrate a 20.00 mL sample of hydrobromic acid...
A 0.080 M NaOH solution was used to titrate a 20.00 mL sample of hydrobromic acid with a concentration of 0.040 M. (a) What is the volume of base needed to reach the equivalence point? (4 pts) (b) What is the pH after adding 7.0 mL of base? (4 pts) (c) What is the pH at the equivalence point? (3 pts)
An aqueous solution of Ca(OH)2with a concentration of 0.161 M was used to titrate 25.00 mL...
An aqueous solution of Ca(OH)2with a concentration of
0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
Part 1 (1 point) How many moles of base were required to react completely with the acid in this reaction? x 10 mol Ca(OH)2 -- Part 2 (1 point) How many moles of HCl were present in the original 25.00 mL of acid? x 10 mol HCl +...
If it requires 24.83 mL of a 0.205 M NaOH solution to titrate a 25.00 mL....
If it requires 24.83 mL of a 0.205 M NaOH solution to titrate a 25.00 mL. HCl solution, what is the concentration of HCI? Type your answer...
If 25.00 mL of 0.500 M NaOH is used to titrate 15.00 mL of H2SO4, what...
If 25.00 mL of 0.500 M NaOH is used to titrate 15.00 mL of H2SO4, what is the molarity of the acid? H2SO4 + 2 NaOH - Na, SO4 + 2 H2O Enter your answer using three significant figures and no units.
A solution of 0.301 M KOH is used to titrate 15.0 mL of a H2SO4 solution....
A solution of 0.301 M KOH is used to titrate 15.0 mL of a H2SO4 solution. Write the balanced equation
answer (2) 2. Suppose that you used a known concentration (0.8442 M) of Ca(OH)2 to determine...
answer (2)
2. Suppose that you used a known concentration (0.8442 M) of Ca(OH)2 to determine the concentration of an unknown HBr solution. If it takes 12.88 mL of the Ca(OH)2 solution to titrate 15.00 mL of the unknown HBr solution, what is the molarity of the HBr? 1. A solid diprotic weak acid, H2A (molecular weight = 128.9 g/mol) is used to standardize a KOH solution. When 0.4228 g of the acid is dissolved in 40.0 mL of water...
stion 62 of 65 > The flask contains 10.0 mL of HCl and a few drops...
stion 62 of 65 > The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.320 M NaOH. It requires 19.4 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? CH concentration: 1.6 M HCI Incorrect 63 of 65 > A barium hydroxide solution is prepared by dissolving 1.67 g of Ba(OH), in water to make 33.6 mL of solution. What is...
7) Titrate 20.0 mL of HNO3 with an unknown concentration with 15.4 mL of 0.300M NaOH. Determine HNO3 concentration. Neutralization equation of nitric acid (HNO3) with NaOH is: HNO3 + NaOH + H2O + NaNO3 8) Titrate 25.00 mL of Ca(OH)2 solution with unknown concentration with 15.65 mL of 1.50M H3PO4. Determine the Ca(OH)2 concentration. Neutralization equation of phosphoric acid with calcium hydroxide is: H3PO4 + Ca(OH)2 + H2O + Ca3(PO4)2 (unbalanced)
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...
A 0.080 M NaOH solution was used to titrate a 20.00 mL sample of hydrobromic acid with a concentration of 0.040 M. (a) What is the volume of base needed to reach the equivalence point? (4 pts) (b) What is the pH after adding 7.0 mL of base? (4 pts) (c) What is the pH at the equivalence point? (3 pts)
An aqueous solution of Ca(OH)2with a concentration of
0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
Part 1 (1 point) How many moles of base were required to react completely with the acid in this reaction? x 10 mol Ca(OH)2 -- Part 2 (1 point) How many moles of HCl were present in the original 25.00 mL of acid? x 10 mol HCl +...
If it requires 24.83 mL of a 0.205 M NaOH solution to titrate a 25.00 mL. HCl solution, what is the concentration of HCI? Type your answer...
If 25.00 mL of 0.500 M NaOH is used to titrate 15.00 mL of H2SO4, what is the molarity of the acid? H2SO4 + 2 NaOH - Na, SO4 + 2 H2O Enter your answer using three significant figures and no units.
answer (2)
2. Suppose that you used a known concentration (0.8442 M) of Ca(OH)2 to determine the concentration of an unknown HBr solution. If it takes 12.88 mL of the Ca(OH)2 solution to titrate 15.00 mL of the unknown HBr solution, what is the molarity of the HBr? 1. A solid diprotic weak acid, H2A (molecular weight = 128.9 g/mol) is used to standardize a KOH solution. When 0.4228 g of the acid is dissolved in 40.0 mL of water...
stion 62 of 65 > The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.320 M NaOH. It requires 19.4 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? CH concentration: 1.6 M HCI Incorrect 63 of 65 > A barium hydroxide solution is prepared by dissolving 1.67 g of Ba(OH), in water to make 33.6 mL of solution. What is...
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