The solution required 28 cm3 of 1 mol dm-3 sodium hydroxide for complete neutralisation. I have calculated moles of moles of NaOH. I am having trouble working out how many moles of acid remained...

The solution required 28 cm3 of 1 mol dm-3 sodium hydroxide for complete neutralisation. I have calculated moles of moles of NaOH. I am having trouble working out how many moles of acid remained...

Help please

What is the molarity of NaOCl in a solution of bleach if 10.00mL requires 22.35mL of 0.02191M Na2S2O3 to reach the endpoint? Show work. Hint: Work through the I2 first. Reaction Equations...

Suppose you did an exploratory titration and 2.00mL of the bleach took 4.60mL of Na2S2O3(aq). How many mL of bleach would you use to end up needing 25-40mL of Na2S2O3(aq)? Round to the nearest mL...

The problem deals with the titration of 441 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.3 M NaOH. How many mL of the 1.3 M NaOH are needed...

The problem deals with the titration of 441 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.3 M NaOH. What will the pH of the solution be when 0.2294...

I just completed a lab in which I titrated Calcium Iodate with Na2S2O3. During the titration we were told to add a starch once the liquid had turned light yellow. When we did this it became dark and...

Q1. Iron is often used to standardize permanganate solutions. A 0.158 g sample of pure iron wire was dissolved in dilute sulfuric acid to form a solution of iron (II) sulfate. This was titrated...

Q1. Iron is often used to standardize permanganate solutions. A 0.158 g sample of pure iron wire was dissolved in dilute sulfuric acid to form a solution of iron (II) sulfate. This was titrated with...

I have absolutely no idea how to do this and do not even know what to search even if I did need help. The question is; If the base solution is 0.250 M and there is one equivalent of OH-...

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 66.2 mL of KOH is __________ M. 0.723 1.00 × 10-7 2.81...

In the titration of 100.0 mL of a 0.0500 M solution of acid H3A (Ka1 = 1.0x10^-3, Ka2 = 5.0x10^-8, Ka3=2.0x10^-12), calculate the volume of 1.00 M NaOH required to reach pH values of 9.50 and 4.00...

It's an acid base titration experiment, where we have to find the concentration of an unown acid using known concentration of a base using indicator. Here we used 0.1 M NaOH, and 5ml H2SO4 made up...

Meredith D.

Tutor with Extensive Special Needs Experience

Baltimore, MD

4.9
(605 ratings)

Med J.

Experienced Biology and Chemistry Tutor

Chicago, IL

4.7
(3 ratings)