Multiple ChoiceWhich of the following solutions will have the lowest concentration of hydronium ions?918views2rank6commentsHas a video solution.
Multiple ChoiceWhich of the following statements about aqueous solutions is/are true?1356views1rankHas a video solution.
Multiple ChoiceWhat is the Kw of pure water at 20.0°C, if the pH is 7.083?1411views4rank5commentsHas a video solution.
Multiple ChoiceCalculate the pH of 50.00 mL of 4.3 x 10-7 M H2SO4.606views2rank5commentsHas a video solution.
Multiple ChoiceDetermine the pH of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a 500.0 mL of solution. (MW of NaCN = 49.01 g/mol). The Ka value of HCN is 4.9 x 10-10.1037views8rank10commentsHas a video solution.
Multiple ChoiceRank the following in order of increasing base strength (weakest to strongest). OI− OCl− OBr−201views
Multiple ChoiceA solution of NaOH was prepared in a chemistry lab and the pOH was determined to be 9.3. What is the concentration of OH− ions of this basic solution?166views4rankHas a video solution.
Multiple ChoiceCalculate [OH−] of a lemon juice solution at 25°C with a [H+] = 5.7 × 10−4 M.180views3rank1commentsHas a video solution.
Multiple ChoiceA 345 mL bottle of antacid (Mg(OH)2) contains 1.45 × 10−2 moles of hydroxide ions. Determine pH and pOH of the antacid.165views4rank3commentsHas a video solution.
Multiple ChoiceWhich of the following statement(s) on aqueous solutions is/are correct?a) aqueous solutions have a pH of 7b) as concentration of hydronium ion increases, concentration of hydroxide ion decreasesc) solutions of weaker acids generally have a higher pOH then solutions of stronger acidsd) pH of pure water equals to 7 at 35º C.163views1rank1commentsHas a video solution.
Textbook QuestionThe probe of the pH meter shown here is sitting in a beaker that contains a clear liquid. (c) Why is the temperature given on the pH meter? 270viewsHas a video solution.
Textbook QuestionWhat is the concentration of hydroxide ions 3OH-4 in a glass of wine with pH = 3.64? (LO 16.5, 16.6) (a) 2.3 * 10-4 M (b) 6.4 * 10-3 M (c) 6.8 * 10-9 M (d) 4.4 * 10-11 M367viewsHas a video solution.
Textbook QuestionCalculate 3H+4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3OH-4 = 8.8 * 10-9 M276viewsHas a video solution.
Textbook QuestionCalculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3H+4 = 2.5 * 10-10 M302viewsHas a video solution.
Textbook QuestionCalculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (c) a solution in which 3H+4 is 1000 times greater than 3OH-4.242viewsHas a video solution.
Textbook QuestionCalculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) 3H+4 = 0.0505 M316viewsHas a video solution.
Textbook QuestionBy what factor does 3H+4 change for a pH change of (a) 2.00 units?267viewsHas a video solution.
Textbook QuestionCalculate [H3O+] and [OH-] for each solution at 25 °C. b. pH = 11.23526viewsHas a video solution.
Textbook QuestionCalculate [H3O+] and [OH-] for each solution at 25 °C. a. pH = 8.551793viewsHas a video solution.
Textbook QuestionCalculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH of an acid solution should carry as many digits to the right of the decimal place as the number of significant figures in the concentration of the solution. [H3O+] = 0.044 M [H3O+] = 0.045 M [H3O+] = 0.046 M1095viewsHas a video solution.
Textbook QuestionDetermine the concentration of H3O+ to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.521847viewsHas a video solution.
Textbook QuestionCalculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (e) -1.0564viewsHas a video solution.
Textbook QuestionCalculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (d) 14.25553viewsHas a video solution.
Textbook QuestionThe equivalence point was reached in titrations of three unknown bases at pH 5.53 (base A), 4.11 (base B), and 6.00 (base C). (a) Which is the strongest base? (b) Which is the weakest base?246viewsHas a video solution.
Open QuestionWhat are the concentrations of H3O+ and OH− in tomatoes that have a pH of 4.10?19viewsHas a video solution.
Open QuestionA solution of ammonia has a pH of 11.8. What is the concentration of OH– ions in the solution?25viewsHas a video solution.
Open QuestionIf the pH of a solution is 7, what is the molar concentration of H+?24viewsHas a video solution.
Open QuestionWhat is the oh ion concentration of an aqueous solution with a pH of 5?19viewsHas a video solution.
Open QuestionThe OH- concentration in an aqueous solution at 25 °C is 6.1 × 10-5. what is [H+]?24viewsHas a video solution.
Open QuestionBleach has a pH of around 12. What is it considered on the pH scale?19viewsHas a video solution.
Open QuestionA solution of HCl has = 0.01 M. What is the pH of this solution? use. –2 –1 1 223viewsHas a video solution.
Open QuestionWhat is the ph of an aqueous solution with the hydronium ion concentration22viewsHas a video solution.
Open QuestionMatch each H+ concentration to its corresponding OH– concentration in aqueous solution.20viewsHas a video solution.