Calculate The PH Value Of HNO3 Solution Containing 0.315 G Acid In ...

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• Calculate the pH value of HNO3...

AnswerQuestion Answers for Class 12Class 12 BiologyClass 12 ChemistryClass 12 EnglishClass 12 MathsClass 12 PhysicsClass 12 Social ScienceClass 12 Business StudiesClass 12 EconomicsQuestion Answers for Class 11Class 11 EconomicsClass 11 Computer ScienceClass 11 BiologyClass 11 ChemistryClass 11 EnglishClass 11 MathsClass 11 PhysicsClass 11 Social ScienceClass 11 AccountancyClass 11 Business StudiesQuestion Answers for Class 10Class 10 ScienceClass 10 EnglishClass 10 MathsClass 10 Social ScienceClass 10 General KnowledgeQuestion Answers for Class 9Class 9 General KnowledgeClass 9 ScienceClass 9 EnglishClass 9 MathsClass 9 Social ScienceQuestion Answers for Class 8Class 8 ScienceClass 8 EnglishClass 8 MathsClass 8 Social ScienceQuestion Answers for Class 7Class 7 ScienceClass 7 EnglishClass 7 MathsClass 7 Social ScienceQuestion Answers for Class 6Class 6 ScienceClass 6 EnglishClass 6 MathsClass 6 Social ScienceQuestion Answers for Class 5Class 5 ScienceClass 5 EnglishClass 5 MathsClass 5 Social ScienceQuestion Answers for Class 4Class 4 ScienceClass 4 EnglishClass 4 MathsCalculate the pH value of \[{\text{HN}}{{\text{O}}_3}\] solution containing \[0.315{\text{ g}}\] acid in \[{\text{200 ml}}\] of solution.\[\left( {{\text{log2}}{\text{.5 = 0}}{\text{.3979 }}} \right)\]A ) 1.6021 B ) 2C ) 0.3979D ) 1AnswerVerified594.3k+ viewsHint: pH of the solution is the negative logarithm of hydrogen ion concentration\[{\text{pH}} = - {\log _{10}}\left[ {{{\text{H}}^ + }} \right]\]For nitric acid solution, the hydrogen ion concentration is equal to the nitric acid concentration. Molarity is the number of moles of solute present in one litre of solution.Complete step by step answer:The molar mass of nitric acid is \[63{\text{ g/mol}}\] . The mass of nitric acid is \[0.315{\text{ g}}\]. Divide mass of nitric acid with its molar mass to calculate the number of moles of nitric acid.\[\dfrac{{0.315{\text{ g}}}}{{63{\text{ g/mol}}}} = {\text{ 0}}{\text{.005 mol}}\]The volume of the solution is \[{\text{200 ml}}\]. Convert the unit of volume from millilitres to litres.\[\dfrac{{200{\text{ mL}}}}{{1000{\text{ L/mL}}}} = {\text{ 0}}{\text{.200 L}}\]Divide the number of moles of nitric acid with the volume of solution to obtain the molarity of nitric acid solution.\[\dfrac{{0.005{\text{ mol}}}}{{0.200{\text{ L}}}} = {\text{ 0}}{\text{.025 M}}\]From the concentration of nitric acid, calculate the concentration of hydrogen ions.\[\left[ {{{\text{H}}^ + }} \right] = \left[ {{\text{HN}}{{\text{O}}_3}} \right] \\\left[ {{{\text{H}}^ + }} \right] = {\text{ 0}}{\text{.025 M}} \\\]Use the concentration of hydrogen ions to calculate the pH of the solution.\[{\text{pH}} = - {\log _{10}}\left[ {{{\text{H}}^ + }} \right] \\ {\text{pH}} = - {\log _{10}}{\text{0}}{\text{.025 M}} \\ {\text{pH}} = - \left( {{{\log }_{10}}\left( {{\text{1}}{{\text{0}}^{ - 2}}{\text{ M}} \times {\text{2}}{\text{.5 M}}} \right)} \right) \\\]\[{\text{pH}} = - \left( {{{\log }_{10}}{\text{1}}{{\text{0}}^{ - 2}}{\text{ M}} + {{\log }_{10}}{\text{2}}{\text{.5 M}}} \right) \\ {\text{pH}} = - \left( { - 2 + 0.3979} \right) \\ {\text{pH}} = - \left( { - 1.6021} \right) \\ {\text{pH}} = 1.6021 \\\]Thus, the pH of the solution is 1.6021.So, the correct answer is “Option A”.Note: Nitric acid is a strong acid. It completely dissociates into aqueous solution to provide hydrogen ions. Usually, the pH of strong acids is in the range 0 to 1.Recently Updated PagesBasicity of sulphurous acid and sulphuric acid areMaster Class 11 Business Studies: Engaging Questions & Answers for SuccessMaster Class 11 Computer Science: Engaging Questions & Answers for SuccessMaster Class 11 Economics: Engaging Questions & Answers for SuccessMaster Class 11 Social Science: Engaging Questions & Answers for SuccessMaster Class 11 English: Engaging Questions & Answers for SuccessBasicity of sulphurous acid and sulphuric acid areMaster Class 11 Business Studies: Engaging Questions & Answers for SuccessMaster Class 11 Computer Science: Engaging Questions & Answers for SuccessMaster Class 11 Economics: Engaging Questions & Answers for SuccessMaster Class 11 Social Science: Engaging Questions & Answers for SuccessMaster Class 11 English: Engaging Questions & Answers for Success

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