Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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What is the equilibrium constant value for NaC2H3O2 and how do you find its Kb?
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- You've just started your summer intern as a research assistant in the biology department. Your first assignment is to prepare a pH 7.50 phosphate buffer solution to be used in the isolation of DNA from a cell culture. You've discovered the following items available to you in the lab: 0.514M HPO 4 (K a-4.2x10 13) 48.6 g KOH (molar mass 56.1g) a. Calculate the pH of your buffer. b. Do you think that this would be a suitable buffer? Explain. SHOW YOUR WORK. Upload your file here.arrow_forwardWhat is the pH of a 0.950 M solution of Na2HPO4? H3PO4 is a weak polyprotic acid with Ka1 = 7.2×10‒3, Ka2 = 6.3×10‒8, and Ka3 = 4.2×10‒13.arrow_forwardHuman blood has a pH of approximately 7.4 due to the carbonic acid/bicarbonate ion (H2CO3/HCO3−) buffer system. Any pH changes below 6.8 or above 7.8 can lead to death! Carbonic acid dissociates to form water and carbon dioxide in the equilibrium shown below. This process is crucial in respiration. H2CO3 (aq) ⇋ CO2 (g) + H2O pKa1 = 2.77 Carbonic acid dissociates in water to form the bicarbonate ion and the hydroxonium ion by the following equilibrium reaction:H2CO3 (aq) + H2O ⇋ H3O(aq)+ + HCO3− pKa2 = 3.70 (i) If there is a 25% increase in carbonic acid levels as per pKa1, explain how the body would deal with this change.arrow_forward
- 4. (a) Calculate [H3O*] and [OH] for the solutions indicated: lemon juice, pH = 2.42 (1) (ii) household ammonia pH = 11.21 (iii) (iv) (v) phosphate buffer pH = 6.96 human urine pOH = 7.8 tomato juice pOH = 9.9arrow_forwardA weak acid is added to a strong base. The base is neutralized last, giving a mole ratio to acid remaining of 2:3. If Ka is 1.0 x 10-5, what is the ph of the solution?arrow_forward5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.arrow_forward
- Consider the following equilibrium: Ag+(aq) + 2 NH3 (aq) ⇌ Ag(NH3)2+ The equilibrium expression is:arrow_forwardWrite the equilibrium constant expression for the formation of FeSCN2+.arrow_forwardCalculate the pH of the solution in which 0.2M NH4Cl and 0.1M NH3 are present. The pKb of ammonia solution is 4.75.arrow_forward
- Calculate the equilibrium concentration (in M) of PO43− that would be present in a mixture that is originally 0.015 M H3PO4 as well as 0.005 M NaH2PO4, given the following information: H3PO4(aq) ↔ H+(aq) + H2PO4−(aq) Ka1 = 1.5 x 10−5 H2PO4−(aq) ↔ H+(aq) + HPO42−(aq) Ka2 = 2.5 x 10−7 HPO42−(aq) ↔ H+(aq) + PO43−(aq) Ka3 = 3.5 x 10−9arrow_forwardWrite the equilibrium constant expression for this reaction: H,CO3(aq) 2H (aq)+CO (aq) →arrow_forwardCoral structures found in the Great Barrier Reef are composed of calcium carbonate, CaCO3, and are under threat of dissolution due to ocean acidification. Consider the following equilibrium reaction equation. CaCO3(s) + CO2(aq) + H2O(l) ⇌ Ca2+(aq) + 2HCO3–(aq) Write the expression for the equilibrium constant, Kc for this reaction. Predict whether the pH of the ocean will increase or decrease as a result of a decrease in the partial pressure of carbon dioxide in the atmosphere (circle your answer). Calculate the molar solubility (s) of calcium carbonate in water at 25 °C when Ksp = 4.5 ´ 10–9.arrow_forward
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