A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 2,421 mL. What is the molarity of nitric acid in the final solution?
A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask
A 20.00 mL, sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 250. mL. What is the concentration of nitric acid in the final solution? 1.27 M 5.08 times 10^-4 M 8.12 times 10^-3 M 0.406 M 3.25 times 10^-2 M A buret is read to how many decimal places? can only be read to the ones place so no decimal places 1 2 4 3
A 25.00 mL sample of nitric acid requires 19.63 mL of 0.1103 M NaOH to reach the end point of the titration. What is the molarity of the nitric acid solution? 0.536 grams of KHP were added to 100.0mL of water. What is the molarity of the KHP solution? (Do not type units with your answer.) Following the procedure for today's lab, a 0.0206 M KHP solution requires 24.59 mL of NaOH solution to titrate it. What is the molarity...
The percentage by weight of nitric acid, HNO3, in a sample of concentrated nitric acid is to be determined. Initially a NaOH solution was standardized by titration with a sample of potassium hydrogen phthalate, KHC8H4O4, a monoprotic acid often used as a primary standard. A sample of pure KHC8H4O4 weighing 1.518 grams was dissolved in water and titrated with the NaOH solution. To reach the equivalence point, 26.90 millilitres of base was required. Calculate the molarity of the NaOH solution....
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH is performed. The pH at 30.00 mL of NaOH added is (a) 1.02 (b) 1.82 (c) 7.00 (d) 3.55 (e) 10.5 18. A titration of 20.00 mL of 0.075 M HNO2 (nitrous acid) with 0.0250 M NaOH is performed. Given that K, for nitrous acid is 4.5 x 104, the pH at 30.00 mL of NaOH added is (a) 1.94 (b) 7.00 (c) 3.35...
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH is performed. The pH at 30.00 mL of NaOH added is (a) 1.02 (b) 1.82 (c) 7.00 (d) 3.55 (e) 10.5
A 14.50 mL sample of nitric acid (HNO3) is titrated to the end point by the addition of 10.45 mL of a 1.525 M solution of barium hydroxide (Ba(OH)2). What is the molarity of the nitric acid solution? (Balanced equation: 2HNO3 + Ba(OH)2 = Ba(NO3)2 + 2 H20)
A 25 mL sample of a 2.0 M solution of MgCl2 is added to a 500 mL volumetric flask. Water is added to the flask until the total volume is 500 mL. What is the concentration of the resulting solution?
need help solving You have 45.0 mL of sample of nitric acid at an unknown concentration. You titrate the sample with 0.1050 M sodium hydroxide and the endpoint is reached at 1285 ml. What was the molarity of the nitric acid solution?
culate the molarity (M) of an unknown solution of hydrochlorie acid (HCT). This experiment similar to the one as done in the lab session.. The acid solution was titrated in a flask with a solution of NaOH added from the buret until the end point (light pink color in the flask) was seen. Followings are the data measured by a student. (3 points) Molarity (M) of NaOH (given) Volume of acid ( measured) in the flask Volume of NaOH required...
10.00 mL Nitric acid was titrated with NaOH of 0.100 molarity until the equivalence was reached. 15.2 mL of NaOH were required. Find: A) Concentration of nitric acid before titration B) pH of solution before titration C) pH of solution after 15.1 mL of sodium hydroxide is added D) pH of solution after 15.3 mL of sodium hydroxide is added