hat is a primary reason for needing to standardize strong base titrants like KOH? Select the single best answer. O KOH is not very soluble in aqueous solutions, thus making the concentrations difficult to determine. KOH reacts with moisture in the air, thereby making accurately-determined concentrations of their solutions difficult. O Standardization is the process of reacting a strong base, like KOH, with an acid. O Standardization is the process of dissolving KOH in aqueous solution. OKOH is a very inexpensive, highly soluble, and easy-to-use base.

hat is a primary reason for needing to standardize strong base titrants like KOH? Select the single best answer. O KOH is not very soluble in aqueous solutions, thus making the concentrations difficult to determine. KOH reacts with moisture in the air, thereby making accurately-determined concentrations of their solutions difficult. O Standardization is the process of reacting a strong base, like KOH, with an acid. O Standardization is the process of dissolving KOH in aqueous solution. OKOH is a very inexpensive, highly soluble, and easy-to-use base.

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.102E

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Three students titrate different samples of the same solution of HCI to obtain its molarity. Below are their data. Student A: 20.00mLHCl+20.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student B: 20.00mLHCl+40.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student C: 20.00mLHCl+20.00mLH2O 0.100 M Ba(OH)2 used to titrate to the equivalence point. All the students calculated the molarities correctly. Which (if any) of the following statements are true? (a) The molarity calculated by A is half that calculated by B. (b) The molarity calculated by A is equal to that calculated by C. (c) The molarity calculated by B is twice that calculated by C. (d) The molarity calculated by A is twice that calculated by B. (e) The molarity calculated by A is equal to that calculated by B.
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Consider the nanoscale-level representations for Question 110 of the titration of the aqueous weak acid HX with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: After a very small volume of titrant has been added to the initial HX solution? When enough titrant has been added to take the solution just past the equivalence point? Halfway to the equivalence point? At the equivalence point? Nanoscale representations for Question 110.
The titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.
Nickel(II) formate [Ni(HCO2)2] is widely used as a catalyst precursor and to make metallic nickel. It can be prepared in the general chemistry laboratory by treating nickel(II) acetate with formic acid (HCO2H). Ni(CH3CO2)2(aq) + 2 HCO2H(aq) Ni(HCO2)2(aq) + 2 CH3CO2H(aq) Green crystalline Ni(HCO2)2 is precipitated after adding ethanol to the solution. (a) What is the theoretical yield of nickel(II) formate from 0.500 g of nickel(II) acetate and excess formic acid? (b) Is nickel(II) formate paramagnetic or diamagnetic? If it is paramagnetic, how many unpaired electrons would you expect? (c) If nickel(II) formate is heated to 300 C in the absence of air for 30 minutes, the salt decomposes to form pure nickel powder. What mass of nickel powder should be produced by heating 253 mg of nickel(II) formate? Are nickel atoms paramagnetic?
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?
5mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl) The Kb for ammonia is 1.75 x 10-5 1)Write a balanced chemical equation for the reaction of ammonia and hydrochloric acid and a balanced chemical equation for the equilibrium of ammonia in water. 2) What is the pH of the ammonia solution prior to the addition of any HCl?
In Dissolution of Borax experiment, the standard HCI solution has a concentration of 0.130 mol/L. The initial buret reading is 4.24, and the final buret reading is 33.38. The volume of the saturated borax solution is 5.34 mL. What is the molar solubility of borax? Note: Report both number and unit. Pay attention to significant figures.
A solution that is 0.00144 M in strontium ion has an aqueous solution of KX added to it slowly. At what concentration of X– will SrX2 begin to precipitate? Ksp (SrX2) = 1.7 × 10–6 Group of answer choices 2.7 × 10–3 5.9 × 10–5 3.4 × 10–2 2.4 × 10–8 1.1 × 10–2
Which one of the following mixture solutions will NOT have a precipitate?Ksp (BaF2) = 1.8 × 10^-7 (Hint: Calculate IP value) A. 100 mL 0.010 M Ba(NO3)2 and 150 mL 0.030 M KF B. 250 mL 0.020 M Ba(NO3)2 and 100 mL 0.010 M NaF C. 150 mL 0.008 M BaCl2 and 100 mL 0.020 M NaF D. 200 mL 0.015 M BaCl2 and 100 mL 0.030 M KF E. 150 mL 0.012 M BaBr2 and 250 mL 0.025 M KF
D. Acid-Base Titrations A 0.1558 g of primary-standard-grade benzoic acid, C6H$COOH, was used to standardize a solution of Mg(OH)2. Calculate the normality of this solution if it needed 19.15 mL of this base to reach the end point of the titration. A solution of an unknown monoprotic acid was found in a laboratory. When titrated, 25.00 mL of this unknown solution needed 28.44 mL of the same base to reach the endpoint. The remaining solution of unknown monoprotic acid amounting 15.00 mL was left in an Erlenmeyer flask uncovered to recover the acid crystals. After 5 days, the mass of the unknown monoprotic acid left on the flask weighed 0.0967 g. Determine the equivalent weight of this unknown acid. FW: C6HSCOOH: 122.12 Mg(OH)2 = 58.32
3a) A student determines the concentration of a sodium hydroxide solution by titration with standardized KHP. S/he obtains the values: 0.190 M, 0.202 M, and 0.205 M. Should the value 0.190 M be rejected? Apply the Q Test. For three values Q must be greater than 0.94 to reject the number. Q = suspect nearest | largest - - smallest b) The student de to repeat the experiment two more The five values now include: 0.190 M, 0.202 M, 0.205 M, 0.201M and 0.203M. Use the Q Test to see if the first value may be rejected. For five values Q must be greater than 0.64 to reject the number. c) Solve for the average Molarity of the measurements from part b with and without the rejected number. Is there value in repeating an experiment several times?