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2. A 50 ml sample required 4.0 ml of 0.02N sulfuric acid to reach the phenoephnophthalein...
Solution 1 (starting material): 4.0 mL of concentrated sulfuric acid is added to a flask, 2.0...
Solution 1 (starting material): 4.0 mL of concentrated sulfuric acid is added to a flask, 2.0 mL of methyl benzoate is then added to the sulfuric acid solution Solution 2 (electrophile, nitronium ion): 2.0 mL of concentrated nitric acid is added to a test tube, followed by 2.0 mL of concentrated sulfuric acid. Add solution 2 to solution 1. Calculate the theoretical yield. concebtration was not given
A 15.44 mL sample of acetic acid requires 32.10 mL of 0.0500 M Ba(OH)2 to reach...
A 15.44 mL sample of acetic acid requires 32.10 mL of 0.0500 M Ba(OH)2 to reach the endpoint. a) Calculate the molarity of the unknown acid b) what is the theoretical pH when 15.8 mL of Ba(OH)2 is added? c) What is the theoretical pH at the point when a total of 32.10 mL Ba(OH)2 is added?
25.000 mL of sodium hydroxide is titrated with 0.100 M sulfuric acid. It requires 15.71 mL...
25.000 mL of sodium hydroxide is titrated with 0.100 M sulfuric acid. It requires 15.71 mL of acid to reach the end point. Calculate the concentration of the base. A. . 159M B. .0628M c. .126M D. .100M how do you do this problem
you are asked to tittate a sample of sulfuric acid of unknown concentration against a standardized...
you are asked to tittate a sample of sulfuric acid of unknown concentration against a standardized solution if sodium hydroxide. you stsrt with 23.00 mL of sulfuric acid in a reaction flask, and 25.67 mL of 1.760 M sodium hydroxide are required to reach the equivalent point, what is the molarity (M) of the sulfuric acid solution? please show conversion steps!
To determine the concentration of a solution of sulfuric acid, a 125.0-mL sample is placed in...
To determine the concentration of a solution of sulfuric acid, a 125.0-mL sample is placed in a flask and titrated with a 0.1433 M solution of cesium hydroxide. A volume of 20.29 mL is required to reach the phenolphthalein endpoint. Calculate the concentration of sulfuric acid in the original sample. A student has 530.0 mL of a 0.1474 M aqueous solution of MnSO4 to use in an experiment. He accidentally leaves the container uncovered and comes back the next week...
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water...
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water and titrated against 0.1555 M NaOH, requiring 48.11 mL to of NaOH to reach the end-point. During the titration reaction, the pH of the solution is 3.77 when half of the HA is neutralized and the equivalence-point pH is 8.33. (a) State two ways to standardize the NaOH used in the titration. (b) Suggest and explain an indicator that can be used in the...
Consider the titration of a 25.0 −mL sample of 0.180 M CH3NH2 with 0.150 M HBr....
Consider the titration of a 25.0 −mL sample of 0.180 M CH3NH2 with 0.150 M HBr. Determine each of the following: a) the initial pH b) the volume of added acid required to reach the equivalence point c) the pH at 4.0 mL of added acid d) the pH at one-half of the equivalence point e) the pH at the equivalence point f) the pH after adding 4.0 mLof acid beyond the equivalence point
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34 mL of a 0.13 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution 16. If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? 17. If 287 mL of 4.7 M HCl solution is added to 284 mL of 3.2 M Ba(OH), solution, what will the pH be? 18. What is...
A 50.0 mL sample of 0.150 M sodium hydroxide is titrated with 0.250 M nitric acid....
A 50.0 mL sample of 0.150 M sodium hydroxide is titrated with 0.250 M nitric acid. Calculate: a. the pH after adding 10.00 mL of HNO3 b. the pH after adding 40.00 mL of HNO3 c. the volume required to reach the equivalence point d. the pH at the equivalence point
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH....
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34 mL of a 0.13 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution 16. If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? 17. If 287 mL of 4.7 M HCl solution is added to 284 mL of 3.2 M Ba(OH), solution, what will the pH be? 18. What is...
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