Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.) a. An aqueous solution of CaO is CaO(ag) + H2O(1) b. An aqueous solution of SO, is SO2 (9) + H20(1) c. An aqueous solution of Cl, O is Cl20(9) + H20(1) >

Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.) a. An aqueous solution of CaO is CaO(ag) + H2O(1) b. An aqueous solution of SO, is SO2 (9) + H20(1) c. An aqueous solution of Cl, O is Cl20(9) + H20(1) >

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

SectionU4.18: Pass The Proton: Acid-base Theories

Problem 8E

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Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
Hydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced equation for the acid-base reaction that could in principle, occur. Does the equilibrium lie toward the products or the reactants?
The pH of 1.0 108 M hydrochloric acid is not 8.00. The correct pH can be calculated by considering the relationship between the molarities of the three principal ions in the solution (H+, Cl, and OH). These molarities can be calculated from algebraic equations that can be derived from the considerations given below. a. The solution is electrically neutral. b. The hydrochloric acid can be assumed to be 100% ionized. c. The product of the molarities of the hydronium ions and the hydroxide ions must equal Kw. Calculate the pH of a 1.0 108-M HCl solution.
Consider the following ions: NH4+, CO32, Br, S2, and ClO4. (a) Which of these ions in water gives an acidic solution and which gives a basic solution? (b) Which of these anions will have no effect on the pH of an aqueous solution? (c) Which ion is the strong base? (d) Write a chemical equation for the reaction of each basic anion with water.
This question has multiple parts.
Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. E Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. Note: =H₂O s of ar rel Ch Solution 1 F (Choose one) R Solution 3 Explanation V (Choose one) ▼ sp 36 5 ▼ T G Check 20 6 Solution 2 (Choose one) (Choose one) Y Solution 4 H 9 7 U J MON B 8 M X D I K ( ² 9 3 O delete return
D Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. Note: Solution 1 (Choose one) 2 = H₂O Explanation Solution 3 (Choose one) ▼ W S ▼ Check 3 747 E D (Choose one) Solution 2 $ (Choose one) 4 Solution 4 R % 5 T X 80 G 6 3 MacBook Pro Y & 7 H © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A U 8 J 1 ( 9 ➡ K ) O O P O
3. Which of the following can act as bases in water and which can act as acids in water: Na2HPO4, CH3OH, Cl2, Ar, Na3AsO4, PbO, C6H14, K2SO4, NH4Cl, NaI, [Fe(H2O)5OH]2-, Al, MnS, CO2 4. Which of the following are soluble salts and which are insoluble salts? NaO2CCH3, S8, Co(OH)2, HCl, C10H22, Ne, CaO, PbCl2, CuSO4×5H2O, BaSO4, NH4Fe3(OH)6(SO4)2, BaCl2, Na2S, K2CO3, Cu2CO3(OH)2
Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. Note: = H,0 Solution 1 Solution 2 hoose one) (Choose one) Solution 3 Solution 4 (Choose one) (Choose one)
Given the following information: nitrous acid = HNO, = CH,COOH acetic acid HNO, is a stronger acid than CH;COOH (1) Write the net ionic equabon for the reaction that occurs when equal volumes of 0.070 M aqueous nitrous acid and sodium acetate are mixed it is not necessany to include states such as (aq) or (8) (2) Which is the strongest base, NO, or CH,CO0 ? (3) At equilibrum the will be favored.
Which statement regarding sulphuric acid is incorrect? a. Concentrated sulfuric acid is about 78% H2SO4 by mass and 10 molar b. It is a strong acid with respect to its first step ionisation c. Its second step ionization is not complete in concentrated solutions d. It is often used as a dehydrating agent because of its strong affinity for H2O
161P.) The ionization constant of a very weak acid, HA, is 1.5×10-9. Calculate the equilibrium concentrations of H3O+, A-, and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O+] = mol/L [A-] = mol/L [HA] = mol/L pH =