Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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What is the equilibrium constant expression for the following reaction?
2 NaHCO3 (aq) ⇌ Na2CO3 (s) + H2O (l) + CO2(g)
Write the concentration equilibrium constant expression for this reaction.
CN (aq) +H₂O(1)→HCN(aq) +OH (aq)
X
0
Ś
010
?
Write the equilibrium constant expression for this reaction:
NH(aq) → NH3(aq) + H+ (aq)
-
x
Ś
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- The 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_forwardCalculate K for the reactions in Question 4.arrow_forwardThe chemistry of gallium: (a) Gallium hydroxide, like aluminum hydroxide, is amphoteric. Write a balanced equation to show how this hydroxide can dissolve in both HCl(aq) and NaOH(aq). (b) Gallium ion in water, Ga3+(aq), has a Ka value of 1.2 103. Is this ion a stronger or a weaker acid than Al3+(aq)?arrow_forward
- The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107arrow_forwardWrite the equilibrium constant expression for this reaction: 2 H (aq) + SO (aq) → H₂SO4(aq) - ? 0 Xarrow_forwardIf the value of K, for HCN is 4.9 x 10-10 at 25 °C, calculate the equilibrium constant for: CN (aq) + H₂O(l)=HCN(aq) + OH (aq) -4.9 x 10-10 O-2.0 x 10-4 4.9 × 10-10 4.9 × 10-16 2.0 × 10-5arrow_forward
- Calculate the pH of each of the following buffered solutions: Ka(HC2H3O2) = 1.8 x 10-5 0.13 M acetic acid/0.23 M sodium acetate 0.23 M acetic acid/0.13 M sodium acetate 0.035 M acetic acid/0.22 M sodium acetate 0.22 M acetic acid/0.035 M sodium acetatearrow_forwardCalculate the pH of each of the following buffered solutions. Ka(HC, HgO,)= 1.8 × 10 5 1.0.19 M acetic acid/0.29 M sodium acetate pH = 2. 0.29 M acetic acid/0.19 M sodium acetate pH = 3. 0.060 M acetic acid/0.21 M sodium acetate pH = 4. 0.21 M acetic acid/0.060 M sodium acetate pH = Visitedarrow_forwardWrite the equilibrium constant expression for this reaction: CH₂OH(aq) + Cl(aq) → CH₂Cl(aq)+OH (aq) X 8 Śarrow_forward
- Consider the following acid/base reaction. What is the Keq (also known as K-equilibrium or equilibrium constant) for this reaction? 10^5 10^11 10^16 10^-11 OH OHarrow_forwardWhat is one acidifying process that produces H+ ions?arrow_forwardWeak Acids dissociate according to the following equation: HA(aq) + H2O(L) ⇌ H3O+ (aq) + A-(aq) In a lab experiment, a student needs to make a buffer solution with a pH of 6.870. If the pKa of the weak acid is 6.500, what ratio of conjugate weak base to acid is needed to make the buffer, I.e. what is the value of [A-/HA]? (Please provide your answer to 3 decimal places.)arrow_forward
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