Titrations are acid-base reactions in which the amount of acid and base in solution are known quite precisely. The specific case wherethe acid and base have been added in equivalent molar amounts, is called the equivalence point. At this point,mol acid = mol base%3DAt all other points in a titration, either the base is the limiting reactant (and there is excess acid) or the acid is the limiting reactant (andthere is excess base). So, except at the equivalence point, titration problems are limiting reactant problems, which means we can dothem- a lot of them!One additional point: when there is left over strong acid (acid in excess), 100% of that excess acid is ionized to become H* ions:[strong acid] = [H*] and pH = -log[H"]Something similar happens for strong bases.1. Calculate the pH of the solution after the following amounts of 0.250 M NaOH have been added to 50.0 mL of 0.200 M HCI. Showall your work for each calculation (including the volumes for which the pH is given). Feel free to attach additional pages to yoursubmission if needed.mL of NaOHpH0.00ANS: 0.69936.0039.7540.0040.2544.0066.00ANS: 12.752. The point at 40.00 mL of NaOH is a turning point in the calculations. How so? What should the pH be at/40.00 mL and why? Howabout after 40.00 mL?

HCl and NaOH react by neutralisation reaction HCl +NaOH→NaCl +H2O. Moles of HCl present =Molarity…

1. Calculate the pH of the solution after the following amounts of 0.250 M NaOH have been added to 50.0 mL of 0.200M HCI. Show all your work for each calculation (including the volumes for which the pH is given). Feel free to attach additional pages to your submission if needed. mL of NaOH pH 0.00 ANS: 0.699 36.00 39.75 40.00 40.25 44.00 66.00 ANS: 12.75

1. Calculate the pH of the solution after the following amounts of 0.250 M NaOH have been added to 50.0 mL of 0.200M HCI. Show all your work for each calculation (including the volumes for which the pH is given). Feel free to attach additional pages to your submission if needed. mL of NaOH pH 0.00 ANS: 0.699 36.00 39.75 40.00 40.25 44.00 66.00 ANS: 12.75

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

See similar textbooks

Similar questions

According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
The equation for a reaction by which a solution of sodium carbonate may be standardized is 2HC7H5O2+Na2CO32NaC7H5O2+H2O+CO2. A student determines that 5.038g of HC7H5O2 uses 51.89mL of sodium carbonate solution in the titration. Find the molarity of the sodium carbonate.
Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
Describe in words the titration of an acid with a base. Be sure to use the terms equivalence point, indicator, and end point correctly.
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is HAsp(aq)+OH(aq)Asp(aq)+H2OWhat is the molar mass of aspirin?
Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture in water, 0.500 M silver nitrate is added dropwise until precipitate formation is complete. The mass of the white precipitate formed is 0.641 g. a. Calculate the mass percent of magnesium chloride in the mixture. b. Determine the minimum volume of silver nitrate that must have been added to ensure complete formation of the precipitate.
Hydrochloric acid. HCl, with a concentration of 0.100 M can be purchased from chemical supply houses, and this solution can be used to standardize the solution of a base. If titrating 25.00 mL of a sodium hydroxide solution to the equivalence point requires 29.67 mL of 0.100 M HCI, what is the concentration of the base?