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Q5) If the mass of the recorded primary standard for standardization of NaOH solution was more than the actual mass, the calculated molarity of the NaOH solution will be:   a) Lower than actual molarity b) As same as actual molarity   c) Exactly as actual molarity d) Higher than actual molarity

Q5) If the mass of the recorded primary standard for standardization of NaOH solution was more than the actual mass, the calculated molarity of the NaOH solution will be:   a) Lower than actual molarity b) As same as actual molarity   c) Exactly as actual molarity d) Higher than actual molarity

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter11: Solutions
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Problem 65AP
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Q5) If the mass of the recorded primary standard for standardization of NaOH solution was more than the actual mass, the calculated molarity of the NaOH solution will be:

 

a) Lower than actual molarity b) As same as actual molarity

 

c) Exactly as actual molarity d) Higher than actual molarity

Q5) If the mass of the recorded primary standard for standardization of NAOH solution was more than the actual mass, the calculated molarity of the NaOH solution will be: a) Lower than actual molarity b) As same as actual molarity c) Exactly as actual molarity d) Higher than actual molarity Q6) Given the following set of data concerning standardization of NAOH solution: - mass of KHP (molar mass = 204.22 g/mol) = 2.97 g - initial burette reading of NaOH = 1.15 mL Final burette reading of NaOH = 30.15 mL The molar concentration of NaOH solution is a) 0.501 M b) 0.050 M c) 0.051 M d) 0.510 M Q7) The indicator that is used for Vitamin C analysis is. a) Phenolphthalein b) I, c) Starch d) KI Q8) A 0.532-g sample of an antacid tablet is dissolved in water. 30.00 mL of 0.141 M HCI solution were added to the sample. The solution is heated and then titrated to the end point with 8.50 mL of a 0.203 M of NaOH solution. The moles of acid that can be neutralized by gram of antacid tablet is a) 0.0047 mol/g b) 0.0025 mol/g c) 4.708 mol/g d) 2.50 mol/g Q9) After adding precise amount of HCl to antacid tablet, the contents of the flask were heated to boiling to a) Dissolve all antacid tablet b) To drive off CO, gas c) To drive the reaction to right d) To keep the content warm
Transcribed Image Text:Q5) If the mass of the recorded primary standard for standardization of NAOH solution was more than the actual mass, the calculated molarity of the NaOH solution will be: a) Lower than actual molarity b) As same as actual molarity c) Exactly as actual molarity d) Higher than actual molarity Q6) Given the following set of data concerning standardization of NAOH solution: - mass of KHP (molar mass = 204.22 g/mol) = 2.97 g - initial burette reading of NaOH = 1.15 mL Final burette reading of NaOH = 30.15 mL The molar concentration of NaOH solution is a) 0.501 M b) 0.050 M c) 0.051 M d) 0.510 M Q7) The indicator that is used for Vitamin C analysis is. a) Phenolphthalein b) I, c) Starch d) KI Q8) A 0.532-g sample of an antacid tablet is dissolved in water. 30.00 mL of 0.141 M HCI solution were added to the sample. The solution is heated and then titrated to the end point with 8.50 mL of a 0.203 M of NaOH solution. The moles of acid that can be neutralized by gram of antacid tablet is a) 0.0047 mol/g b) 0.0025 mol/g c) 4.708 mol/g d) 2.50 mol/g Q9) After adding precise amount of HCl to antacid tablet, the contents of the flask were heated to boiling to a) Dissolve all antacid tablet b) To drive off CO, gas c) To drive the reaction to right d) To keep the content warm
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