Interpretation:
The concentration of hydronium
Concept introduction:
At a particular temperature, the product of concentrations of water is called the ionic product of water and it is denoted by
Water is a universal solvent and it is a weak electrolyte. Based on the self-ionization of two moles of water, molecules combine to form hydronium ions
At
The concentrations of hydronium and hydroxide ions are equal in a neutral solution.
By using the equilibrium expression,
Rearrange the above equation for hydronium ions as:
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Chemistry
- practice pH a.) determine the pH of a nitric acid solution (HNO3) that has been prepared by mixing 2.0 mL of 1.0 M HNO3 with 98.0 mL of water b.) determine the pH of a 25 mL carbonic acid solution (H2CO3) with concentration of 5.7 x 10-5 M. assume all protons will dissociate from the acid and react with water to form hydronium ions. c.) determine the pH and pOH of a NaOH solution that has been prepared by diluting 20.0 mL of 6.0 M NaOH with 80.0 mL of water. d.) determine the pH and pOH of a Ca(OH)2 solution that has been prepared by mixing 0.26 g of Ca(OH)2 pellets in 750 mL of water.arrow_forwardExercise 6b. Arrange the solutions in order of increasing acidity: NaCl, NH4CI, KCN, NaOH, NaCH3COO, NaC3H5O3, Nicotine, C2H5NH3Cl HA and HB are both weak acids in water, and HA is a stronger acid than HB. Which of the following statements is correct? A) A is a stronger base than B, which is a stronger base than H₂O, which is a stronger base than Cl-. B) B is a stronger base than A, which is a stronger base than H₂O, which is a stronger base than Cl-. C) B is a stronger base than A, which is a stronger base than Cl, which is a stronger base than H₂O. D) CI is a stronger base than A, which is a stronger base than B, which is a stronger base than H₂O. E) None of these (A-D) is correct.arrow_forwardConsider the following beakers. Each contains a solution of the hypothetical atom X. a Arrange the beakers in order of increasing concentration of X. b Without adding or removing X, what specific things could you do to make the concentrations of X equal in each beaker? (Hint: Think about dilutions.)arrow_forward
- Exercise 1 Calculate the pH of each of the following solutions: (a) 0.63 M NaCH3CO2(aq), K, = 5.62 × 10-10, %3D (b) 0.19 M NH4CI(aq), K, = 5.6 × 10-10; %3D (c) 0.65 M KCN(aq), K½ = 2 × 10-5.arrow_forwardA solution has [OH- ] = 4.0 x 10-8. What is the value of[H+] for the solution?(a) 2.5x 10 -8 M (b) 4.0 x 10 -8 M (c) 2.5 x 10 -7 M(d) 2.5 x10 -6 M (e) 4.0 x 10 -6 Marrow_forwardPractice Exercise The pH of a certain orange juice is 3.33. Calculate the H* ion concentration.arrow_forward
- Exercise 3. ldentify all the Bronsted acids and bases in the following equations: (a) NH3 + HCI NH,* + CH (b) HSO; + CN- HCN + SO,- (c) H,PO, + CO;- HPO,2- + HCO;arrow_forwardPractice Exercise What is the pH of a solution containing 0.30 M HCOOH and 0.52 M HCOOK? Compare your result with the pH of a 0.30 M HCOOH solution.arrow_forwardKnowledge check. Based on the fact that NaOH is a strong base and C₆H₈O₇ is a weak acid, how would you describe the pH of the solution at the endpoint, where moles of base = 3 times the moles of acid? A) strongly basic pH B) weakly basic pH C) neutral pH D) weakly acidic pH E) strongly acidic pHarrow_forward
- What is the pH of a 0.420 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)? Answer is not 9.43 or 11.16arrow_forwardQUESTION7 Which solution below has the highest concentration of hydroxide ions? o pH = 7.00 o pH = 12.49 O pH = 7.93 O pH = 10.12 O pH = 3.21 QUESTION 8arrow_forwardWhat is the pH of a 0.25 M solution of H3PO4? Ka = 7.2 x 10-³ (A) 0.25 (B) 7.2 x 10-3 (C) 0.0018 (D) 0.042 (E) 1.37arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning