A 25.00 mL solution containing 0.035 M sodium acetate is titrated with a 0.098 M solution...
1 Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000443 mol KIO30.0000443 mol KIO3 were titrated with an unknown solution of Na2S2O3 and the endpoint was reached after 17.80 mL17.80 mL. How many moles of Na2S2O3 did this require? 2. How many moles are present in a 25.00 mL sample of 0.076 M acetate? 3. A 25.00 mL solution containing 0.035 M sodium acetate is titrated with a 0.098 M solution of HCl. How many...
Question 6 Status: Tries remaining: 3 | Points possible: 1.00 Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000460 mol KIO3 were titrated with an unknown solution of Na S,0a and the endpoint was reached after 17.80 mL. How many moles of Na,S203 did this require? Answer: CHECK Question 8 Status: Tries remaining: 3 | Points possible: 1.00 A 25.00 mL solution containing 0.035 M sodium acetate is titrated witha 0.098 M solution of HCl....
6) A 35 mL solution of 0.241 M HCl is titrated with 0.127 M NaOH: a) How many milliliters of NaOH solution are required to reach the equivalence point? b) What is the pH at the midpoint of the titration? c) What is the pH at the endpoint of the titration?
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 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.04328 M EDTA solution. The solution is then back titrated with 0.02246 M Zn2 solution at a pH of 5. A volume of 21.60 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the...
18. A 25.00 ml sample of the 50.00 ml solution was titrated with 0.1359 M potassium thiocyanate and 12.90 mL were required to reach the endpoint. Calculate the gram of silver (MM= 107.87 g/mol) in the sample.
A 1.000-mL aliquot of a solution containing Cu and Ni2 is treated with 25.00 mL of a 0.05182 MEDTA solution. The solution is then back titrated with 0.02198 M Zn2 solution at a pH of 5. A volume of 21.82 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu and Ni2 solution is fed through an ion-exchange column that retains Ni2. The Cu2 that passed through the column is...
5. A 25.00 ml. sample of H.SO, istitrated against a 0.752 M NO solution 271 ml of the 0.752 M NaOH solution is required to reach the endpoint of the stration, calculate the concentration of the H.SO, solution: 6. How many mL of a 0.322M Mg(OH), solution would be needed to bitrate 25.00 mL of a 0.575 M HCI solution?
1) A 25.00 mL sample of HBr is titrated with a 0.150 M standardized sodium hydroxide solution. The endpoint was reached when 18.80 mL of titrant had been added. Calculate the molar concentration of the HBr.
You titrated a 25.00 mL solution of 0.02 M oxalic acid with a freshly prepared solution of KMnO4. If it took 41.81 mL of this solution to reach the endpoint, what was the molarity of the KMnO4? 0.0119 is wrong +/- 3 sig figs.