Calculate the volume of 0.106 M NaOH needed to neutralize a 50.00 mL sample of 0.0950 M HNO3.
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Calculate the volume of 0.106 M NaOH needed to neutralize a 50.00 mL sample of 0.0950...
Question 3 Question 3 - 6 pts Calculate the volume of 0.106 M NaOH needed to neutralize a 50.00 mL sample of 0.0950 M HNO 44.81 ml 50.35 mL 55.79 mb 201 mL
Calculate the pH of a mixture of 51.0 mL of 0.106 M NaOH and 50.00 mL of 0.0950 M HNO3.
A 50.00 mL sample of 0.0950 M acetic acid (Ka = 1.8 x 10-5) is being titrated with 0.106 M NaOH. What is the pH at the half-way point of the titration? (22.41 mL of 0.106 M NaOH has been added) A) 3.06 B) 5.04 C) 4.44 D) 3.18 E) 4.74
What volume of a 0.442 M NaOH solution is needed to neutralize 65.0 mL of a 0.296 M solution of HNO3? O 43.5 mL O 87.1 mL O 21.8 mL O 174 mL O 8.71 mL
What volume of 0.060 M HCl will completely neutralize 50.00 mL of 0.2400 M NaOH? S. 12.5 mL B. 25 mL C. 100 mL D. 200 mL
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/
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.
how many mL of 0.250 M NaOH are needed to completely react with 50.00 mL of 0.400 M HNO3? NaOH + HNO3 => NaNO3 + H2O