Multiple ChoiceWhich of the following solutions will have the lowest concentration of hydronium ions?986views2rank6comments
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 10-10.1115views8rank10comments
Multiple ChoiceRank the following in order of increasing base strength (weakest to strongest). OI− OCl− OBr−285views
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?233views5rank
Multiple ChoiceCalculate [OH−] of a lemon juice solution at 25°C with a [H+] = 5.7 × 10−4 M.262views5rank1comments
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.229views5rank3comments
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.255views2rank1comments
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? 352views
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 M473views
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 M371views
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 M393views
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-4.337views
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 M408views
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 M1219views
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 = 2.522001views
Textbook QuestionCalculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (e) -1.0673views
Textbook QuestionCalculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (d) 14.25679views
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?347views
Open QuestionA solution of ammonia has a pH of 11.8. What is the concentration of OH– ions in the solution?103views
Open QuestionThe OH- concentration in an aqueous solution at 25 °C is 6.1 × 10-5. what is [H+]?110views
Open QuestionMatch each H+ concentration to its corresponding OH– concentration in aqueous solution.93views