Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A B C H₂O H₂O, NaOH H₂O, NaOH H₂O initial type (check all that apply) acidic basic neutral acidic basic neutral acidic sic neutral acidic basic neutral 0 000 000 00 change add H Br add NaNO3 add HNO3 add K Br effect of change on pH (check one) ο οοίο ο ο1ο ο ο X pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same S

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A B C H₂O H₂O, NaOH H₂O, NaOH H₂O initial type (check all that apply) acidic basic neutral acidic basic neutral acidic sic neutral acidic basic neutral 0 000 000 00 change add H Br add NaNO3 add HNO3 add K Br effect of change on pH (check one) ο οοίο ο ο1ο ο ο X pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same S

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 70AP

See similar textbooks

Similar questions

One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
Assume that a sample of hard water contains 50. mg/L of Mg2+ and 150 mg/L of Ca2+, with HCO3 as the accompanying anion. What mass of CaO should be added to 1.0 L of this aqueous solution to precipitate all the Mg2+ and Ca2+ as CaCO3 and MgCO3? What is the total mass of the two solids formed?
A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
Which of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to fine particles before dissolving. c. The temperature changes.
In Exercise 12.49, what is the allowed concentration of AgCl in g per 100 g of water? The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mgofsolute/L of solution.)
Suppose that an aqueous solution is in equilibrium with solid calcium sulfate and solid barium sulfate. What are the concentrations of calcium ion and barium ion in the solution?
For the simple reaction 2H2(g)+O2(g)2H2O(l)list the types of bonds that must be broken and the types of bonds that must form for the chemical reaction to take place.
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type solution initial components (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral A B 09 C D H₂O H₂O H₂O, HCIO H₂O, HCIO4 0000000 change add HI add KI add NaClO add NaOH effect of change on pH (check one) O pH higher O pH lower OpH the same O pH higher O pH lower OpH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A C H₂O H₂O, HNO3 H₂O H₂O, HNO3 initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral change add NaOH add KNO3 add NaCl add KOH effect of change on pH (check one) pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A B C D H₂O H₂O, NaOH H₂O H₂O, NaOH initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic оо 00 neutral change add HCl add Na Br add K Cl add H Br effect of change on pH (check one) pH higher pH lower ο ο1ο ο ο ο ο ο pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A B с H₂O H₂O, NaOH H₂O, NaOH H₂O initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral change add KI add NaBr add H Br add HI effect of change on pH (check one) pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same