Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Formic acid, HCOOH, is the simplest of the carboxylic acids and occurs naturally, most notably in some ants. If the formate (HCOO–) concentration is 0.100 M, determine the formic acid (HCOOH) concentration required to buffer a solution at pH = 3.35 HCOOH(aq) ↔ HCOO–(aq) + H+(aq) Ka = 1.80 × 10-4 i) Calculate the pKa of the acid and provide your final answer with 3 decimal places ii) Write the main equation that you will use to help you calculate the formic acid concentration iii) Calculate the formic acid concentration required to buffer the solution at pH = 3.35 and provide your final answer with 3 decimal placesarrow_forwardCalculate the hydronium ion concentration in an aqueous solution of 0.293 M carbonic acid, H2CO3 (aq).[H3O+] = M.arrow_forwardA Dashboard 101 Chem101 + а ap.101edu.co Question 10 of 16 Submit Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH:(aq) + HCI(aq) - 14- O3- |2+ 3+ 14+ 1 2 3 4 7 9. 1 I5 16 (s) (g) (aq) H3O+ H2O OH- CI Reset • x H2O Delete + 10:24 PM P Type here to search 65°F Mostly sunny 10/31/2021 1Larrow_forward
- Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.400 M phosphoric acid solution. pKa1 pKa2 pKa3 2.16 7.21 12.32 [H3PO4]= M [H+]= M [H2PO4−]= M [OH−]= M [HPO2−4]= M pH= [PO3−4]= Marrow_forwardCalculate K₂ or K from experimental data. The pH of a 0.14-M solution of chlorous acid (HCIO₂) is measured to be 1.49. Use this information to determine a value of Ka for chlorous acid. HCIO₂(aq) + H₂O(l)=CIO₂ (aq) + H₂O˚(aq) K₂ =arrow_forwardThe acid dissociation constant K of boric acid (H₂BO3) is 5.8 × 10-¹0. Calculate the pH of a 5.6M solution of boric acid. Round your answer to 1 decimal place. pH = 0 X 6arrow_forward
- Calculate the concentration of HC6H₁06 in an aqueous solution of 4.81x10-2 M ascorbic acid, H₂C6H6O6 (aq). [HC6H606] = M.arrow_forwardA monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) ⇒ H+ (aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] A¯] = 3.00 × 10-4 M. Calculate the value of pK₁ for the acid HA. a pK₂: a = = 0.240 M, [H+] = 3.00 × 10−4 M, andarrow_forwardConsider a buffer solution that consists of two separate components: the weak acid, CH3COOH(aq), and its conjugate base, CH3COO¯ (aq) (added as NaCH3COO). Which component will react with H+(aq) from a strong acid? Write the net ionic equation for the reaction that occurs when H+(aq) is added to the buffered solution. Which component will react with OH-(aq) from a strong base? Write the net ionic equation for the reaction that occurs when OH-(aq) is added to the buffered solution.arrow_forward
- Acetylsalicylic acid (aspirin), HC₂H7O4, is the most widely used pain reliever and fever reducer. What is the equilibrium concentration of all species, the pH, % ionization, and pOH of a 0.0187 M solution of aspirin? K₁ = 3.60 x 10-4arrow_forwardYou are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth. Y2O + Y2O ⇌ Y3O+ + OY– Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths placearrow_forwardCalculate the pH at 25 °C of a 0.23 M solution of sodium hypochlorite (NaClO). Note that hypochlorous acid (HCIO) is a weak acid with a pK, of 7.50. a Round your answer to 1 decimal place. pH = 0 ?arrow_forward
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