In a titration experiment, 11.5 mL of 0.400 M H2SO4 neutralized 48.0 mL of NaOH. What was the concentration of the NaOH solution?
In a titration experiment, 11.5 mL of 0.400 M H2SO4 neutralized 48.0 mL of NaOH. What...
Question 19 6 pts In a titration, 3.54mL of NaOH is neutralized using 14.60 mL of 0.150 M H2SO4. What is the concentration of the NaOH solution in molarity? (Report your answer without units)
In a titration experiment, 11.7 mL of an aqueous H2SO4 solution was titrated with 0.4 M NaOH solution. The equivalence point in the titration was reached when 10.7 mL of the NaOH solution was added. What is the molarity of the H2SO4 solution? H2SO4 molarity
In a titration experiment, 9.3 mL of an aqueous H2SO4 solution was titrated with 0.3 M NaOH solution. The equivalence point in the titration was reached when 9.9 mL of the NaOH solution was added. What is the molarity of the H2SO4 solution?
In a titration of 22.41mL of 0.1237 M H2SO4, 37.25 mL of NaOH solution are needed. What is the concentration of the NaOH solution?
50 mL solution of 0.2 M H2SO4 is titrated until neutralized with 25 mL NaOH. Calculate the molarity of NaOH solution.
100.0 mL of 0.400 M aqueous NaOH and 50.00 mL of 0.400 M aqueous H2SO4, each at 24.00°C, were mixed, see equation: 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) The final temperature achieved by the solution was 26.65 °C. Neglect the heat capacity of the cup and the thermometer, and assume that the solution of products has a density of exactly 1.00 g/mL and specific heat capacity of 4.18 J/(g•C) How much heat did the reaction release?
What is the molarity of an H2SO4 solution if 35.00 mL is exactly neutralized by 32.63 mL of 0.164 M NaOH? 2NaOH + H2SO4---> Na2SO4 + 2H20
A 65.0 mL sample of 1.0 M NaOH is mixed with 48.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 24.4°C. After adding the NaOH solution to the coffee cup, the mixed solutions are stirred until reaction is complete. Assume that the density of the mixed solutions is 1.0 g/mL, that the specific heat of the...
You titrate 50.0 mL of 0.400 M HClO4 (a strong acid) with 0.400 M NaOH. a. Write the balanced equation. b. What is the pH at the beginning of the titration (0.0 mL of NaOH)? c. What is the pH after adding 30.0 mL of NaOH? d. At the equivalence point, is the pH greater than, less than, or equal to 7.00? Explain briefly.
A 25.00 mL sample of NaOH was titrated with a 0.743 M H2sO, solution. The endpoint of the titration was observed after the addition of 5.00 ml. of H2SO4. Calculate the concentration of the NaOH 2. solution.