Hey there! We receieved your request
Stay Tuned as we are going to contact you within 1 Hour
One of our academic counsellors will contact you within 1 working day.
Click to Chat
1800-5470-145
+91 7353221155
Use Coupon: CART20 and get 20% off on all online Study Material
Complete Your Registration (Step 2 of 2 )
Sit and relax as our customer representative will contact you within 1 business day
OTP to be sent to Change
Calculate the concentration of nitric acid in moles per litre in a sample whichhas a density, 1.41 g mL–1 and the mass per cent of nitric acid in it being 69%.
Mass percent of nitric acid in the sample = 69 % [Given]
Thus, 100 g of nitric acid contains 69 g of nitric acid by mass.
Molar mass of nitric acid (HNO3)
= {1 + 14 + 3(16)} g mol–1
= 1 + 14 + 48
= 63 g mol–1
∴ Number of moles in 69 g of HNO3
Volume of 100g of nitric acid solution
Concentration of nitric acid
∴Concentration of nitric acid = 15.44 mol/L
given: 1.41 g/mL HNO3 solutionthe solution is 69% HNO31. calculate the mass of HNO3 in the solution= 1.41 g/ml x 69%= 0.9729 g/ml 2. convert the answer in 1 to mole quantity by dividing it with the molar mass of HNO3 which is 63 g/mol= 0.9729 g/ml divided 63 g/mol= 0.01544 mol/ml3. Since molar quantity is expressed as mole per L, you need to multiply the answer in 2 with 1000 (1L = 1000ml)= 0.01544 mol/ml X 1000 = 15.44 MThe concentration of the solution is 15.44 M.
Get your questions answered by the expert for free
You will get reply from our expert in sometime.
We will notify you when Our expert answers your question. To View your Question
Win Gift vouchers upto Rs 500/-
Register Yourself for a FREE Demo Class by Top IITians & Medical Experts Today !