Answered: If a solution containing 66.97 g of… | bartleby

Introductory Chemistry For Today

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.109E

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Question

Assuming complete precipitation, how many
moles of each ion remains in solution? If an
ion is no longer in solution, enter a zero (0) for
the number of moles. I submitted something
similar earlier, mol for C2H3O2- was wrong.
Having trouble figuring it out.
C2H3Ò2-
If a solution containing 66.97 g of mercury(II) acetate is allowed to react completely with a solution containing 10.872 g of
sodium sulfide, how many grams of solid precipitate will be formed?
mass:
How many grams of the reactant
excess will remain after the reaction?
mass:
Assuming complete precipitation, how many moles of each ion remain
(0) for the number of moles.
solution?
an ion is no longer in solution, enter a zero
Hg2+:
mol
CH,0;:
mol
Na*:
mol
s2-:
mol

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As a result of contamination by atmospheric carbon dioxide, a sodium hydroxide solution contains a small amount of sodium carbonate. To reach the phenolphthalein end point, a 25.00-mL aliquot requires 27.75 mL of 0.1021 M HCl and an additional 1.61 mL to reach the methyl red end point. Calculate the molar concentration of NaOH in the solution.
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A 250.0-mg sample of an organic weak acid is dissolved in an appropriate solvent and titrated with 0.0556 M NaOH, requiring 32.58 mL to reach the end point. Determine the compound’s equivalent weight.
if you do a standardization titration using and unknown molarity of NaOH to neutralize the above 25mL of KHP (0.098mol) , and you came to the equivalent point. How many moles of NaOH were neutralized?
The reaction of KOH with HNO2 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq)---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (HNO2) when 40.5 mL of 0.674 M KOH is required to quench 101.0 mL of Nitric acid over phenolphthalein indicator.
In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question
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