1. A certain experiment requires 624.0 mL of 0.00445 M NaOH.
i). Calculate the number of grams of NaOH required to make this solution.
ii). Calculate the mass percentage of a 0.00445 M NaOH solution (the density of solution is 1.52 g/mL).
iii). Calculate the pOH and pH of this 0.00445 M NaOH solution.
iv). What volume of 0.175 M NaOH solution is required to make 624.0 mL of 0.00445 M NaOH solution?
v). Calculate the pOH and pH of the following mixture: 43.7 mL of a 0.18 N H2SO4 solution after it is mixed with 57.3 mL of a 0.35 N NaOH solution.
1. A certain experiment requires 624.0 mL of 0.00445 M NaOH. i). Calculate the number of...
NaOH requires to prepare 250 mL of a NaOH solution 0.100 M Preparation of a 0.1 M NaOH solution: Calculate how much (in grams) of NaOH is required to prepare 250 mL of a NaOH solution 0.100 M. CALCULATIONS:
A solid weak acid is weighed, dissolved in water and diluted to exactly 50.00 ml. 25.00 ml of the solution is taken out and is titrated to a neutral endpoint with 0.10 M NaOH. The titrated portion is then mixed with the remaining untitrated portion and the pH of the mixture is measured. Mass of acid weighed out (grams) 0.773 Volume of NaOH required to reach endpoint: (ml) 19.0 pH of the mixture Ihalf neutralized solution 3.54 Calculate the following...
1. What volume of 0.10 M NaOH is needed to neutralize 100 mL of 0.050 M HCl? 2a. When 100 mL of 0.01 M NaOH solution is mixed with 100 mL of 0.01 M of HNO3 solution, what is the concentration of H+ and the pH in the resulting mixture? 2b. When 100 mL of 0.01 M NaOH solution is mixed with 100 mL of 0.02 M of HCl solution, what is the concentration of H+ and the pH in...
4. A solution of 0.200 M NaOH (14.0 mL) is mixed with 42.4 mL of o.170 M HNO,. Assuming that the final volume is the sum of the initial volumes, calculate: (a) the molarity of the Na* cation (b) the molarity of the NO, anion (c) the pH of the final solution (d) the pOH of the final solution
45.00 mL of a 0.250 M H2SO4 solution is titrated with 0.100 M NaOH. a. What is the chemical equation that describes this neutralization reaction? b. What is the volume in mL of NaOH required to reach the equivalence point? c. At the equivalence point, what are the sodium and sulfate ion concentrations? d. At the equivalence point, what are the pH and pOH
5 5 of the (original) mixture is titrated with 0.100 M NaOH. How many ml of this base c. 100.0 ml must be added to just reach a pH of 5.50 for the solution? Also determine d. Another 100.0 mL of the (original) mixture is mixed with 70.0 mL of 0.100 M NaOH. Determine the pH of the solution at this point. (Note that ascorbit acid is diprotic.) [H2Ab]-? o.Ou .o64 2. 400.0 mL of 0.100 M H2Ab (ascorbic a...
A 25.01 mL sample of H2SO4 solution requires 34.31 mL of 0.3643 M NaOH. What is the molarity of the H2SO4 solution? Type your answer
A 27.41 mL sample of H2SO4 solution requires 34.34 mL of 0.3274 M NaOH. What is the molarity of the H2SO4 solution? Type youp answer... Previous
It requires 38.23 mL of 0.7500 M NaOH solution to completely neutralize 155.6 mL of an aqueous solution of sulfuric acid. What is the concentration (mol/L) of the H2SO4 solution?
A 108.2 mL sample of 1.00 M NaOH is mixed with 54.1 mL of 1.00 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 23.05 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 30.50 °C. Assume that the density of the mixed solutions is 1.00...