To neutralize 100cm3 of 0.2M sulfuric acid you
need:
a)200cm3 of 0.2M Ba(OH)2
b)100cm3 of 0.1M Ba(OH)2
c)80cm3 of 0.25M Ba(OH)2
d)80cm3 of 0.50M Ba(OH)2
To neutralize 100cm3 of 0.2M sulfuric acid you need: a)200cm3 of 0.2M Ba(OH)2 b)100cm3 of 0.1M...
1) 10ml of 0.1M Nitric Acid is added to 20ml of 0.2M Sulfuric (H2SO4) and then diluted up to 100 ml, what is the resulting pH? Hint: Recall [H3O+] = total moles of [H+]/total Volume 2) Which of the following acid solutions is the MOST acidic? (careful it’s a mix of concentrations as well as Ka and pKa) a) 1.0M Phenol, Ka = 1.3 x 10-10 b) 0.08M Pyruvic acid, pKa = 2.76 c) 0.1M Bromo-Acetic acid pKa =...
a. Calculate the volume of 0.450 M Ba(OH), which will be needed to neutralize 46,00 mL of 0.252 M HCI. b. Find the molar concentration of a sulfuric acid solution, 35.00 mL of which neutralizes 25.00 mL of 0.320 M NaOH. (Careful! Sulfuric acid is diprotic!) c. Calculate the "molarity of water" H₂O in pure water at 30°C. (Hint: The density of water at 30°C is 0.9957 g/mL.] d. A 15.00 mL sample of a solution of H₂SO₄ of unknown concentration was titrated with...
How many moles of HNO3HNO3 are present if 7.80×10−2 molmol of Ba(OH)2Ba(OH)2 was needed to neutralize the acid solution?
Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium hydrogen carbonate on it and then mopping up the resultant solution. The sodium hydrogen carbonate reacts with sulfuric acid producing sodium sulfate, water, and carbon dioxide. Sodium hydrogen carbonate is added until the fizzing due to the formation of carbon dioxide stops. If 27.0 mL of 5.4 M sulfuric acid was spilled, what is the minimum mass of sodium hydrogen carbonate that must...
How many moles of HNO3 are present if 4.60×10−2 mol of Ba(OH)2 was needed to neutralize the acid solution?
How many moles of HNO3 are present if 6.10×10−2 mol of Ba(OH)2 was needed to neutralize the acid solution?
What volume of 0.1292 M Ba(OH)2 would neutralize 50.00 mL of 0.1000 M HCl solution? Ba(OH)2(aq) + 2HCl(aq) ⟶ BaCl2(aq) + 2H2O(l)
5. Sodium bicarbonate (baking soda) will neutralize sulfuric acid according to the following reaction: 2 H200) + 2 CO2()+ Na2SOs(aq) 2 NAHCO3(aq)+H2SO4(aq) If a student spills 250.0 mL of sulfuric acid, how many grams of sodium bicarbonate should they use in order to completely neutralize it? Assume the density of sulfuric acid is 1.84 g/m L.
What volume (in mL) of 0.100 M barium hydroxide, Ba(OH)b, is needed to completely neutralize 25.0 mL of 1. 0.100 M hydrochloric acid, HCI? (A) 12.5 mL (C) 50.0 ml What are the Bronsted-Lowry bases in this reaction? (B) 250 mL (D) 75.0 mL 2. NH,(aq) + H2O(l) 근 NH'(aq) + OH-(hq) (B) HO and NH4 D) NH. and OH (A) NH and OH (C) NH, and H.O 3. What is the conenration of hydroxide ion in 0.015 M HCI(aq)...
In the next reaction, what is the acid? a. HCN b. Ba (OH) 2 c.H2O d. Ba (CN) 2 2HCN (ac) + Ba(OH)2 (ac) → 2H2O (/) + Ba(CN)2 (ac)