Chemistry
posted by Savannah .
A solution of NaOH with pH 13.68 requires 35.00 mL of 0.128 M HClO_4_ to reach the equivalence point. How do you calculate [Na^+^] and [ClO_4_^^] at the aquicalence point? (volumes are additive)

We've been here before. What's the problem? You have M NaOH (from the pH = 13.68), you have mL HClO4 and you have M HClO4. There is only one unknown in
mL NaOH x M NaOH = mL HClO4 x M HClO4.
Respond to this Question
Similar Questions

Chemistry
A 40.00 mL sample of 0.1 M NH3 is titrated with 0.150 M HCl solution. Kb = 1.8 * 10^5 What volume of base is required to reach the equivalence point? 
Chemistry
A few questions I don't really get and need to see the work for A 50.0 mL sample of 0.55 M benzoic acid, C6H5COOH, a weak monoprotic acid, is titrated with 0.51 M NaOH. Calculate the pH at the equivalence point. Ka of C6H5COOH = 6.5 … 
Chemistry
I really don't know how to approach this problem and I really need help. Using the average molarity of your initial acetic acid solutions, the initial volumes, and the volume of NaOH added to reach the equivalence point, calculate … 
Chemistry
In this case, the inflection point, and equivalence, occurs after 23.25mL of 0.40 M NaOH has been delivered. Moles of base at the equivalence point can be determined from the volume of base delivered to reach the equivalence point … 
chemistry
A solution of NaOH with pH 13.68 requires 35.00 mL of 0.128 M HClO_4_ to reach the equivalence point. What is the volume of the NaOH solution? 
Chemistry
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (a) 100.0 mL of 0.14 M HC7H5O2 (Ka= 6.4 multiplied by 105) titrated by 0.14 M NaOH halfway point equivalence point (b) 100.0 … 
chemistry
A volume of 100mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence … 
chemistry
a sample of 20.0 mL of 0.100 M HCN (Ka=6.2*10^10) is titrated with 0.150 M NaOH. a) what volume of NaOH is used in this titration to reach the equivalence point? 
Chemistry
The number of moles NaOH needed to reach the equivalence point is mol, which means we must add liters of NaOH. The total volume of solution at the equivalence point will be liters. From the above information, the molarity of NaF at … 
Chemistry
A titration involves titrating 0.4 M NaOH into a solution of 0.2 M H3PO4. a.) Calculate the volume of NaOH that will be required to reach the first equivalence point. b.) Calculate the volume of NaOH required to reach the second equivalence …