Molarity = number of moles of solute x 1000 / volume of solution (mL)
or, number of moles of solute = Molarity x volume of solution (mL) / 1000
number of moles of solute NaOH = 0.200 x 1700 / 1000
number of moles of solute NaOH = 0.34 mole
Calculate the miles of NaOH present in 1700 ml of a solution 0.200M NaOH.
A 20.0mL sample of 0.200M HBr is titrated with 0.200M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: a. 15.0mL b. 35.0mL
25. If 10.00 mL of 0.200M HCl is added to 30.0 mL of 0.0500 M NaOH, what is the pH of the solution? Show all work for full credit. (6 pts)
A student titrates a 22.0mL solution of 0.200M HCN with 0.200M NaOH The acid disse HCN is 6.2x10-10 Of The acid dissociation constant of 1. Determine the pH of the acetic acid solution before any NaOH is added 2. Determine the pH of the solution when 6.00mL of 0.100M NaOH has been added. 3. Determine the pH of the solution when17 OmL of 0.100M NaOH has been added. 4. Determine the pH of the solution at the equivalence point.
Calculate the grams of NaOH present in 10.0 mL of a 8.0% (m/v) NaOH solution. 8.0 g 0.80 g 0.72 g 7.2 g Question 8 Which of the following solutions has a molarity of 2.0? 0.020 mole of solute in 50.0 mL of solution 3.0 moles of solute in 3.0 L of solution 0.050 mole of solute in 25.0 mL of solution 2.0 moles of solute in 500.0 mL of solution
A student titrates a 22.0mL solution of 0.200M HCN with 0.200M NaOH. The acid dissociation constant of HCN is 6.2 x 10^(-10) Determine the pH of the acetic acid solution before any NaOH is added. Determine the pH of the solution when 6.00mL of 0.100M NaOH has been added Determine the pH of the solution when17.0mL of 0.100M NaOH has been added. Determine the pH of the solution at the equivalence point Determine the pH of the solution after an...
100. ml of 0.200M HCl is titrated with 0.250M NaOH. 1. What is the pH of the solution after 50.0ml of base has been added? 2.What is the pH of the solution at the equivalence point?
Consider a 100mL buffer solution prepared to be 0.200M HC2H302 and 0.200M KC2H302. Calculate the pH of the buffer system after 0.0040 mol of NaOH are added. A. 4.569 B. 4.921 C. 7.00 D. 11.602 The correct answer is B, but I need to show my work which I am not sure how to do.
Calculate the number of moles os sodium hydroxide (NaOH) present in 42.0 mL of a 0.629 M NaOH solution. Please round your answer to the ten-thousandth place. Dony express your answer in scientific notation. Thank you.
Calculate the concentration (in molarity) of an NaOH solution if 25.0 mL of the solution is n neutralize 18.9 mL of a 0.239 M HCl solution.
Calculate the concentration (in molarity) of an NaOH solution if 25.0 mL of the solution is needed to neutralize 15.5 mL of a 0.305 M HCl solution.