Answer:
105mL of 0.7500M of NaOH are required
Explanation:
Phosphoric acid, H₃PO₄, reacts with sodium hydroxide, NaOH, as follows:
H₃PO₄ + 3 NaOH → Na₃PO₄ + 3H₂O
<em>Where 1 mole of phosphoric acid reacts with 3 moles of NaOH</em>
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To solve this question we must find, as first, the moles of H3PO4 that react. Using the chemical equation we can find the moles of NaOH required to neutralize this acid. And, with its concentration, we can find the volume oof NaOH required:
<em>Moles H3PO4:</em>
35.00mL = 0.03500L * (0.7500mol / L) = 0.2625 moles H3PO4
<em>Moles NaOH:</em>
0.2625 moles H3PO4 * (3mol NaOH / 1mol H3PO4) = 0.07875 moles NaOH
<em>Volume NaOH:</em>
0.07875 moles NaOH * (1L / 0.7500mol) = 0.105L =
<h3>105mL of 0.7500M of NaOH are required</h3>
Answer:
0.95mol
Explanation:
1mole of NH3 contains 6.02x10^23 molecules
Therefore, Xmol of NH3 will contain 5.70x10^23 molecules i.e
Xmol of NH3 = (5.70x10^23) /6.02x10^23 = 0.95mol
Answer:
P₂ ≅ 100 atm (1 sig. fig. based on the given value of P₁ = 90 atm)
Explanation:
Given:
P₁ = 90 atm P₂ = ?
V₁ = 18 Liters(L) L₂ = 12 Liters(L)
=> decrease volume => increase pressure
=> volume ratio that will increase 90 atm is (18L/12L)
T₁ = 272 Kelvin(K) T₂ = 274 Kelvin(K)
=> increase temperature => increase pressure
=> temperature ratio that will increase 90 atm is (274K/272K)
n₁ = moles = constant n₂ = n₁ = constant
P₂ = 90 atm x (18L/12L) x (274K/272K) = 135.9926471 atm (calculator)
By rule of sig. figs., the final answer should be rounded to an accuracy equal to the 'measured' data value having the least number of sig. figs. This means P₂ ≅ 100 atm based on the given value of P₁ = 90 atm.
Answer:
<u>The new pressure is 1.0533 atm</u>
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Explanation:
According to<u> Boyle's Law :</u> The Pressure of fixed amount of gas is inversely proportional to Volume at constant temperature.
PV = Constant
P1V1 = P2V2
.....(1)
P1 = 3.16 atm
Accprding to question ,
V1 = V
V2 = 3 V
Insert the value of V1 , V2 and P1 in the equation(1)
V and V cancel each other
