i need help with understanding 7a,7b, and 7c A 2 M NaOH is used to titrate...
An aqueous solution of Ca(OH)2with a concentration of 0.143 M was used to titrate 25.00 mL of aqueous HCl. 14.73 mL of the Ca(OH)2was required to reach the endpoint of the titration. How many moles of base were required to react completely with the acid in this reaction? How many moles of HCl were present in the original 25.00 mL of acid? What is the molarity of the original HCl solution? 04 Question (a points) aSee page 166 Watch the...
this is my prelab for class, I'm really struggling to understand so if someone could help me break down the problems that would be nice Experiment 12 THE DETERMINATION OF THE NEUTRALIZING ABILITY OF ANTACIDS The Pre-Lab 1. A 1.032 gram sample of an antacid was dissolved in 50 mL of water. Then a 49.33 mL portion of 0.488 M HCI was added to the flask. The antacid was completely neutralized and the unneutralized hydrochloric acid remaining in the flask...
this is my prelab for class, I'm really struggling to understand so if someone could help me break down the problems that would be nice Experiment 12 THE DETERMINATION OF THE NEUTRALIZING ABILITY OF ANTACIDS The Pre-Lab 1. A 1.032 gram sample of an antacid was dissolved in 50 mL of water. Then a 49.33 mL portion of 0.488 M HCI was added to the flask. The antacid was completely neutralized and the unneutralized hydrochloric acid remaining in the flask...
Question 3 3 pts 3. A 2.5 M HCl solution is used to titrate (neutralize) a 5.0 M NaOH solution. a. How many ml of the HCI solution would be needed to "neutralize" 400 ml of the 5.0 M NaOH?? (think C1V1=C2V2) b. Write the balanced equation for the reaction of HCI with NaOH c. In the above equation which you just wrote, identify the conjugate acid and the conjugate base Upload Choose a File
you want to titrate a 0.10 l of 0.20 m naoh. However, you are given a 0.50 l solution of h3po4 of unknown concentration. It takes 0.25 l solution of 0.25 L solution of 0.25 m Ca(oh)2 to neutralize the H3Po4 solution. Find the concentration of the h3po4 solution and then calculate how many litres of the original h3po4 solution is needed to fully neutralize the naoh solution
Questions 3, 4, & 5 pls (3) You will titrate a solution of an unknown acid (HX(aq)) by adding NaOH(aq). Suppose that 25 mL of 0.5 M NaOH(aq) is needed to reach the equivalence point. How many moles of HX were present initially? Show the calculation. (4) You will titrate acid solutions by adding 0.2-0.3-mL or 2-3-mL portions of NaOH(aq). When should you add the smaller volume? (5) The concentration of an aqueous solution of NaOH cannot be accurately determined...
35.25 mL of NaOH solution are required to titrate 0.5745 g of an unknown monoprotic acid. Prior standardization of the NaOH determined its concentration as 0.1039 M. 1. Use the data provided to determine the molar mass of the unknown acid 2. If 20 mL of a 1.0 M solution of the unknown monoprotic acid is placed into a beaker and 10 mL of 0.1 M NaOH is added, the pH of the final solution is 1.9. What is the...
Molarity for NaOH = 0.08732. In a second titration with the same solution of NaOH as used in Question #1, the student weighs out a sample of KHP of 0.359 g. Calculate the volume of the NaOH solution needed to neutralize this sample of KHP. 3. A monoprotic weak acid with the general formula of HA will react with a base, such as NaOH. Write the neutralization equation which describes the reaction. 4. If K, for the weak acid, HA is 1.8...
A solution of 0.12 M NaOH is used to titrate 55.0 mL 0.28 M HCI. Determine the concentration of NaCl in the resulting solution at the equivalence point. Periodic Table Constants and Factors Supplemental Data Acid Dissociation Constants Base Dissociation constants
If 25.0 mL of 0.150 M NaOH were used to titrate a solution of H2SO4, how many grams of H2SO4 are present in the solution?