A 25 mL solution of nitric acid, HNO3, required 31.1 mL of 0.1459 M NaOH to reach a bromthymol blue end point. What is the concentration of the nitric acid solution?
A 25 mL solution of nitric acid, HNO3, required 31.1 mL of 0.1459 M NaOH to...
42.04 mL of a solution of the acid HNO3 is titrated, and 52.40 mL of 0.5500-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.
If 9.91 mL of an Acetic acid solution required 10.43 mL of 1.0628 M NaOH to reach the end point , whats the concentration of an acetic acid?
A 25.00 mL sample of nitric acid requires 19.63 mL of 0.1103 M NaOH to reach the end point of the titration. What is the molarity of the nitric acid solution? 0.536 grams of KHP were added to 100.0mL of water. What is the molarity of the KHP solution? (Do not type units with your answer.) Following the procedure for today's lab, a 0.0206 M KHP solution requires 24.59 mL of NaOH solution to titrate it. What is the molarity...
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH is performed. The pH at 30.00 mL of NaOH added is (a) 1.02 (b) 1.82 (c) 7.00 (d) 3.55 (e) 10.5
A 14.50 mL sample of nitric acid (HNO3) is titrated to the end point by the addition of 10.45 mL of a 1.525 M solution of barium hydroxide (Ba(OH)2). What is the molarity of the nitric acid solution? (Balanced equation: 2HNO3 + Ba(OH)2 = Ba(NO3)2 + 2 H20)
1. if 15.27 mL of 0.250 M solution of barium hydroxide is required to reach the equivalence point in a titration of 20.00 mL of nitric acid, what is the concentration of the acid? The equation for the reaction is 2 HNO3 + Ba(OH)2 --> 2 H2O + 2 NO3- + Ba2+ 2. For the reaction: HCOOH + OH- --> HCOO- + H2O If 24.60 mL of base is required to reach the equivalence point of this titration, what volume...
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH is performed. The pH at 30.00 mL of NaOH added is (a) 1.02 (b) 1.82 (c) 7.00 (d) 3.55 (e) 10.5 18. A titration of 20.00 mL of 0.075 M HNO2 (nitrous acid) with 0.0250 M NaOH is performed. Given that K, for nitrous acid is 4.5 x 104, the pH at 30.00 mL of NaOH added is (a) 1.94 (b) 7.00 (c) 3.35...
Titration of 25.00 mL of an unknown diprotic acid solution required 15.09 mL of 0.10 M NaOH to reach the first equivalence point and 29.82 mL of 0.10 M NaOH to reach the second equivalence point. What is the concentration of the diprotic acid solution?
If 9.16 mL of an acetic acid solution required 9.45 mL of 1.0841 M NaOH to reach the endpoint, what's the concentration of the acetic acid solution?
If 10.24 mL of an acetic acid solution required 9.02 mL of 1.0821 M NaOH to reach the endpoint, what's the concentration of the acetic acid solution?