NAME DATE SECTION PoS POSTLABORATORY ASSIGNMENT I. A sodium hydroxide solution i
ID: 916528 • Letter: N
Question
NAME DATE SECTION PoS POSTLABORATORY ASSIGNMENT I. A sodium hydroxide solution is standardized using 0.500 g of solid oxalic acid, H C,o Find the molarity of the base if 33.50 mL are required for the titration to a phenolphthalein endpoint. HX2049 2 NaOH(aq) + NayC204 (aq) 2H20(1) + 2. A 10.0-mL sample of household ammonia solution required 33.25 mL. of 0.345 M HCI to reach neutralization. Calculate (a) the molar concentration of the ammonia and (b) the mass/mass percent concentration of ammonia (17.04 g/mol), given a solution density of 0.980 g/mL HCI (aq) NH3(aq) NH4Cl (aq) + 3. If 27.50 ml of 0.200 M nitric acid is required to neutralize 25.0 ml of barium hydroxide solution, what is the molar concentration of the base? Ba(NO3)2(aq) 2H2O(i) + Ba(OH)2(aq) 2 HNO3(aq) + Analysis of VinegarExplanation / Answer
1.
Molar mass of Oxalic acid = 90.03 g·mol1
wt. of Oxalic acid = 0.5 g
mol= wt. of oxalic acid/ molar mass of oxalic acid= 0.5/90.03= 0.00555 mol
H2C2O4 (s) + 2 NaOH (l) ------> Na2C2O4 (aq) + 2 H2O (l)
1 mole of H2C2O4 reacts with 2 mole of NaOH
0.00555 mole of H2C2O4 requires 0.0111 mole of NaOH
Number of moles = Molarity X volume in Liters,
0.0111 mole of NaOH= Molarity x 0.0335 L or
Molarity of NaOH= 0.3313 M
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