Write the balanced NET IONIC equation for the reaction that occurs when hydrobromic acid and calcium hypochlorite are combined. Use H30* instead of H*. (aq) (aq) (aq) : This reaction is classified as c. A. Strong Acid + Strong Base B. Weak Acid + Strong Base C. Strong Acid + Weak Base D. Weak Acid + Weak Base The extent of this reaction is: A. A. Below 50% B. 50% C. Above 50% D. 100%

Write the balanced NET IONIC equation for the reaction that occurs when hydrobromic acid and calcium hypochlorite are combined. Use H30* instead of H*. (aq) (aq) (aq) : This reaction is classified as c. A. Strong Acid + Strong Base B. Weak Acid + Strong Base C. Strong Acid + Weak Base D. Weak Acid + Weak Base The extent of this reaction is: A. A. Below 50% B. 50% C. Above 50% D. 100%

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section: Chapter Questions

Problem 109GQ: (a) What is the pH of a 0.105 M HCl solution? (b) What is the hydronium ion concentration in a...

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Common Acids and Bases Use the data in Table 18.8 to answer the following questions. Which substance is the most basic? Which substance is closest to neutral? Which has a concentration of H+=4.01010M ? Which has a pOH of 11.0? How many times more basic is antacid than blood?
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Figure 14.3 shows the pH of some common solutions. How many times more acidic or basic is each of these compared with a neutral solution? (a) Milk (b) Seawater (c) Blood (d) Battery acid
(a) What is the pH of a 0.105 M HCl solution? (b) What is the hydronium ion concentration in a solution with a pH of 2.56? Is the solution acidic or basic? (c) A solution has a pH of 9.67. What is the hydronium ion concentration in the solution? Is the solution acidic or basic? (d) A 10.0-mL sample of 2.56 M HCl is diluted with water to 250. mL What is the pH of the dilute solution?
35. For each pair of concentrations, tell which represents the more acidic solution. a. [H+]=1.2103Mor[H+]=4.5104M b. [H+]=2.6106Mor[H+]=4.3108M c. [H+]=0.000010Mor[H+]=0.0000010
Using your results from Exercise 133, place the species in each of the following groups in order of increasing base strength. a. OH, SH, SeH b. NH3, PH3 c. NH3, HONH2
Find [H+] and the pH of the following solutions. (a) A 456-mL sample of a 12.0% (by mass) solution of HNO3(d=1.00g/mL). What is the pH of 10.0 mL of the same sample? (b) A solution made up of 1.0 g of HCI dissolved in enough water to make 1.28 L of solution. What is the pH of the solution? If the same mass of HCI is dissolved in enough water to make 128 mL of solution, what would the pH be?
Use Table 14.3 to help order the following acids from strongest to weakest HNO3,H2O,NH4+,C5H5NH+
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?
Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. Li2O b. CO2 c. SrO
Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic. The relevant Ka and Kb values are found in Tables 13-2 and 13-3. a. NaNO3 b. NaNO2 c. C5H5NHClO4 d. NH4NO2 e. KOCl f. NH4OCl
Which of the following statements is correct about the reaction below? HAsO42- (aq) + H2O (liq) → AsO43- (aq) + H3O+ (aq) a. HAsO42- is an acid and H2O is its conjugate base. b. HAsO42- is a base and AsO43- is its conjugate acid. c. H2O is an acid and AsO43- is its conjugate base. d. HAsO42- is an acid and AsO43- is its conjugate base. e. HAsO42- is an acid and H3O+ is its conjugate base.

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