This can easily be solved by using normality equation as discussed N1V1=N2V2
O.106 × V = 0.0950 × 50.00
V = (0.0950×50.00)÷0.106
= 4.750 ÷ 0.106
= 44.811 ml
Therefore the first option is correct.
Question 3 Question 3 - 6 pts Calculate the volume of 0.106 M NaOH needed to...
Calculate the volume of 0.106 M NaOH needed to neutralize a 50.00 mL sample of 0.0950 M HNO3.
Calculate the pH of a mixture of 51.0 mL of 0.106 M NaOH and 50.00 mL of 0.0950 M HNO3.
Post-Laboratory Questions 1. Calculate the volume of a 0.200 M NaOH solution needed to neutralize 40.0 mL of 0.600 M HNO, solution. 2. Calculate the volume of a 0.200 M KOH solution needed to neutralize 40.0 mL of a 0.600 M H,SO, solution.
Calculate the volume of 0.510-M NaOH solution needed to completely neutralize 26.5 mL of a 0.860-M solution of the diprotic acid H2C2O4.
Calculate the volume of 0.660-M NaOH solution needed to completely neutralize 49.6 mL of a 0.460-M solution of the diprotic acid H2C2O4.
A) What is the volume of 0.700 M NaOH needed to neutralize the 20.00 mL of 1.30 M HC1 solution? b) The data suggest a different volume was needed to neutralize the HCI. Explain why this may be the case.
Part A. Calculate the volume lf 0.210-M NaOH solution needed to completely neutralize 89.1 mL of a 0.310-M solution of the diprotic acid H2C2O4 Part B. You wish to make a 0.202 M Hydrochloric acid solution from a stock solution of 3.00 M hydrochloric acid. How much concdntrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution? Part C. an aqueous solution of barium hydroxide is standarized by titration with a 0.143 M...
50 ml sample of 0.0950 M acetic acid (ka: 1.8* 10-5) isbeing titrated with 0.106 M NaoH. 1- what is the PH at the midpoint of titration? 2- what is the PH equivalence point of the titration? 3-what is the PH and endpoint of titration/
1) How many milliliters of a 0.100 M NaOH solution are needed to neutralize 15.0 mL of 0.200 M H₃PO₄? 2) If 24.7 mL of 0.250 M NaOH solution are needed to neutralize 19.8 mL of H₂SO₄, solution, what is the molarity of the H₂SO₄? 3) 25.0 g of 5.0% (by mass) acetic acid solution are titrated with 0.300 M NaOH. What volume of NaOH will be needed to neutralize this sample?
2) If 24.7 mL of 0.250 M NaOH solution are needed to neutralize 19.8 mL of H,SO, solution, what is the molarity of the H,SO 2Nadd tuSot Naso2H20 24 NOS 25.0 g of 5.0 % ( by mass ) acetic acid solution are titrated with 0.300 M NaOH. What volume of NaOH will be needed to neutralize this sample? 3)