Answer:
Solution 1 has a higher pH at the equivalence point because CH3CO2H has the stronger conjugate base.
Explanation:
Since according to the chemical reaction shown below, if the conjugated base is stroboscopic, the product of the reaction would be an OH- so that its pH is higher:
CH3COO- + H2O = CH3COOH+ OH-
Answer:
is there any answer choices????
1) Calculate the number of moles in 1.15 liter of 0.100 M HNO3 solution.
M = n / V => n = M*V = 0.100M * 1.15 l = 0.115 moles
2) Calculate the mass of 0.115 moles of HNO3
mass = number of moles * molar mass
molar mass of HNO3 = 1.00 g/mol + 14.0 g/mol + 3*16.0g/mol = 63.0 g/mol
mass = 0.115 mol * 63.0g/mol = 7.245 g
3) Calculate the mass of 70.3% HNO3 solution that contains 7.245 grams of HNO3
% = (mass of solute / mass of solution) * 100
=> mass of solution = mass of solute * 100 / % = 7.245 g * 100 / 70.3%
mass of soltuion = 10.3 g.
4) Convert 10.3 grams of HNO3 solution into volume, using density, D
D =mass / Volume => Volume = mass / D
=. Volume = 10.3 g / 1.41 g/cm^3 = 7.30 cm^3
Answer: 7.30 cm^3
Answer:
a. 1.728 moles.
b. 262.7g of Cr₂O₃ are required
Explanation:
Based on the reaction:
Cr₂O₃(s) + 3H₂S(g) → Cr₂S₃(s) + 3H₂O(l)
The important thing in the reaction is that 1 mole of Cr₂O₃ produce 1 mole of Cr₂S₃
a. To produce 346g of Cr₂S₃ we must know how many moles of Cr₂S₃ must be produced, and, as 1 mole of Cr₂O₃ produce 1 mole of Cr₂S₃ we can know moles of Cr₂O₃ that are required.
<em>Moles of 346g Cr₂S₃ (Molar mass: 200.19g/mol):</em>
346g Cr₂S₃ * (1mol / 200.19g) = 1.728 moles of Cr₂S₃
Based on the reaction, moles of Cr₂O₃ that are required are
<h3>
1.728 moles of Cr₂O₃</h3>
b. Again, to conver the 1.728 moles of Cr₂O₃ to grams we must use molar mass of Cr₂O₃ (151.99g/mol):
1.728 moles Cr₂O₃ * (151.99g / mol) =
<h3>262.7g of Cr₂O₃ are required</h3>