How much water would you need to add to 10.0 mL of 0.500 M HCl to...

Question

Question

science chemistry

Answer 1

Answer #1

10XS we know from litration - Ws, a Vg Sy - here V, = 10 ml, S, = 0.5M 2 Viso = OKS 225 me, 1. V ?? S2 = 0.2 M.. so, Total

Answer 2

Similar Homework Help Questions

If I mixed 100.0 mL of a nitric acid solution of pH = 2.40 with 100.0...

If I mixed 100.0 mL of a nitric acid solution of pH = 2.40 with 100.0 mL of a nitric acid solution of pH = 2.70, what would be the pH of the mixture? Write your answer to 2 digits beyond the decimal (e.g., 8.63) If 5.15 grams of iron(III) nitrate (molar mass = 241.86 g/mol) is dissolved in enough water to prepare exactly 150.0 mL of solution, what would be the molar concentration of the nitrate ion? 0.284 M...
What volume of a 0.500 M HCl solution is needed to completely neutralize 10.0 mL of...

What volume of a 0.500 M HCl solution is needed to completely neutralize 10.0 mL of a 0.200 M Ba(OH)2 solution? Ba(OH)2(aq) + 2 HCl(aq) → BaCl2(aq) + 2 H2O(l) a. 10.0 mL b. 4.00 mL c. 2.00 mL d. 8.00 mL
1.) If 15.0 mL of 3.60 M HCl (aq) are added to 10.0 mL of water,...

1.) If 15.0 mL of 3.60 M HCl (aq) are added to 10.0 mL of water, what is the concentration of the resulting solution? 2.) How many mL of water must be added to 25.0 mL of a 0.500 M NaCl solution to result in a solution that is 0.200 M NaCl? 3.) The net ionic equation for the reaction of aqueous solutions of sodium chloride and silver nitrate is...? 4.) How many mL of a 0.500 M sodium chloride...

11. How much water would I need to add to 200 mL of a 1.4 M...

11. How much water would I need to add to 200 mL of a 1.4 M KCl solution to bring the molarity to 1 M? (Read question carefully)
27.64 ml of 0.500 M HCl is required to titrate 10.0 ml of barium hydroxide solution....

27.64 ml of 0.500 M HCl is required to titrate 10.0 ml of barium hydroxide solution. what is the concentration of the barium hydroxide solution?
You add 16.00 mL of 0.600 M NaOH to 50.00 mL of pure water, and to...

You add 16.00 mL of 0.600 M NaOH to 50.00 mL of pure water, and to this mixture you then add 100 ml of 0.300 M HCI. What will be the pH of the resulting solution? You add 7.50 mL of 0.050 M NaOH to 50.00 mL of pure water, and to this mixture you then add 1.50 mL of 0.200 HCI. What will be the pH of the resulting solution? o 11.89 o o o

You add 9.00 mL of 0.200 M NaOH to 50.00 mL of pure water, and to...

You add 9.00 mL of 0.200 M NaOH to 50.00 mL of pure water, and to this mixture you then add 12.00 mL of 0.600 M HCI. What will be the pH of the resulting solution?
You add 9.00 mL of 0.200 M NaOH to 50.00 mL of pure water, and to...

You add 9.00 mL of 0.200 M NaOH to 50.00 mL of pure water, and to this mixture you then add 19.00 mL of 0.700 M HCL What will be the pll of the resulting solution?
A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the...

A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 27.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 MM CH3COOH (Ka=1.8×10−5Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 15.0 mL of NaOH. and Imagine that you are in chemistry lab and need to make 1.00 LL of a solution with a pH of 2.80. You have in front...

You add 1.00 mL of 0.300 M NaOH to 50.00 mL of pure water, and to...

You add 1.00 mL of 0.300 M NaOH to 50.00 mL of pure water, and to this mixture you then add 16.00 mL of 0.800 M HCI. What will be the pH of the resulting solution You add 16.00 mL of 0.600 M NaOH to 50.00 mL of pure water, and to this mixture you then add 100 mL of 0.300 M HCL What will be the pH of the resulting solution?