Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Complete the balanced molecular reaction for the following weak acid with a strong base:
HNO2(aq) + Ca(OH)2(aq) ->
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- Complete each of these reactions by filling in the blanks. Predict whether each reaction is product-favored or reactant-favored, and explain your reasoning. (a) _________ (aq) + Br(aq) NH3(aq) + HBr(aq) (b) CH3COOH(aq) + CN(aq) ________ (aq) + HCN(aq) (c) ________ (aq)+H2O () NH3(aq) + OH(aq)arrow_forwardOne 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?arrow_forwardThe simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)arrow_forward
- An aqueous solution contains a mixture of 0.0500 M HCOOH (Ka = 1.77 104) and 0.150 M CH3CH2COOH (Ka = 1.34 105). Calculate the pH of this solution. Because both acids are of comparable strength, the H+ contribution from both acids must be considered.arrow_forwardThe hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.arrow_forward8) What is the pH of a 0.035 M HNO, solution? HNO3 (aq) + H,0 (1) H;O* (aq) + NO; (aq)arrow_forward
- Write the equilibrium constant expression for this reaction: H;PO,(aq) - 3 H (aq)+PO (aq) ?arrow_forwardWaste acid of pH 3.0 is stored in a lead-lined vessel, as shown in the figure below. If the walls of the container undergo corrosion by the following reaction: Pb(s) + 2H*(aq) → Pb*"(aq) + H;(g) what is the equilibrium concentration of dissolved Pb-* at 25°C if the pressure of hydrogen gas in the closed vessel is 0.5 atm? The AG; for Pb (aq) is –5,810 cal/mol. Waste acid pl- 30 Lead-lined tunkarrow_forwardA phosphate buffer contains KH2PO4 and K2HPO4. What is the net ionic equation for the buffering reaction that occurs when some HCl is added to the buffer solution? (A) H2PO4–(aq) + Cl–(aq) --> HPO42–(aq) + HCl(aq); (B) H2PO4–(aq) + H3O+(aq) --> H3PO4(aq) + H2O(aq); (C) HPO42–(aq) + Cl–(aq) --> PO43–(aq) + HCl(aq); (D) HPO42–(aq) + H3O+(aq) --> H2PO4–(aq) + H2O(aq);arrow_forward
- A weak acid has a Ka of 7.6 x 106. What is the value of pk for the acid? a pKa =arrow_forwardIn the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HCIO, (aq) + H,O(1) = H,O*(aq) + CI0, (aq) H,CO, (aq) + H,O1) – H;O*(aq) + HCO; (aq) Answer Bank H,O(1) + CH;NH†(aq) = CH,NH,(aq) + H;O*(aq) СА А B СВ CH, COOH(aq) + H,O(1) - CH;COO (aq) + H;O*(aq)arrow_forwardWhich of the followingarrow_forward
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