A 0.311 g of antacid was neutralized with 50.0 mL of 0.102 M HCI. Calculate the neutralizing capacity of antacid? a. 0.00255 mol HCl/g antacid b. 0.00328 mol HCl/g antacid c. 6.55 mol HCl/g antacid d. 16.4 mol HCl/g antacid e. 0.0164 mol HCl/g antacid

QUESTION 4 A 50.0-mL sample of a 1.50  M NaOH solution is titrated with a 1.56  M HCl solution. What will be the final volume of solution when the NaOH has been completely neutralized by the HCl?   a. 167 mL   b. 83.1 mL   c. 48.1 mL   d. 2.7 mL   e. 98.1 mL

1. A student is given two solutions of hydrochloric acid, HCl (a monoprotic acid), but with different concentrations. Which statement is true? a. There is no chemical method designed to tell the two solutions apart. b. It would take more NaOH solution (base solution), per milliliter of the unknown solution, to neutralize the more concentrated HCl solution. c. A smaller volume of the less concentrated solution contains the same number of moles of the acid compared to the more concentrated solution. d. If the same volume of each sample was taken, then more base solution would be required to neutralize the one with lower concentration. e. The product of concentration and volume of the less concentrated solution equals the product of concentration and volume of the more concentrated solution.

5.00 mL of 1.00 M HCl is added to a flask containing antacid powder dissolved in water. The solution is then titrated with 0.20 M NaOH, and the titre volume recorded is 17.85 mL.  How many mol of HCl was neutralised by the antacid tablet?     Select one: a. 0.0014 mol HCl b. 0.80 mol HCl c. 0.0036 mol HCl

Get two medium test tubes. Into one, place about 2 mL of a solution of hydrochloric acid. Into the other add a small amount of solid sodium carbonate. Note the appearances of the contents in the two test tubes and then mix them together noting any changes that have taken place. what changes take place? whats the balanced equation? whats the ionic? whats the net ionic

Chem. 1011 Lab Acid/Base neturatlization Worksheet 3 9. If it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solution, what is the concentration of the NaOH solution? 10. If it takes 50 mL of 0.5 M Ca(OH)2 solution to completely neutralize 125 mL of sulfuric acid solution (H2SO4), what is the concentration of the H2SO4 solution? 11. How many milliliters of 0.360 M H2SO4 are required to neutralize 25.0 mL of 0.100 M Ba(OH)2?

1. If 10. g of AgNO3 is available, what volume of 0.40 M AgNO3 solution can be prepared? Volume =   mL? 2. A 7.52-g sample of a diprotic acid requires 179.0 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.  g/mol?

What is a neutralization reaction? Write one example for it.

What best sums up Le Chatelier's principle is  A. According to this, a system in balance tends to change in a way that releases tension while under stress.  B. Le Chatelier's principle can be applied in several situations, such as when you blow air through a straw or dissolve an alka-seltzer pill in a glass of water.  C. explains how acids are created and destroyed, and how anything can operate to raise the concentration.  D. All of the above

Emma titrated 20.00 mL of an HCL(aq) solution that has an unknown concentration with 0.1240 M NaOH(aq). The equivalence point is reached after adding 25.46 mL of NaOH(aq).   a. Write out the complete balanced equation for the reaction that occurs in this titration. b. How many moles of NaOH were added to the HCl solution? c. How many moles of HCl were in the original 20.00 mL solution? d. What was the concentration of HCl in the original 20.0 mL solution?