Kelvin
When measuring in kelvin units the lowest unit is 0k
The mass of the gas dissolved in 1.00 L of water at 25°C and 3.0 atm is equal to 1.26 grams.
<h3>How to determine the
mass of the
gas dissolved?</h3>
In order to determine the mass of the gas dissolved, we would the calculate the new (final) solubility of this gas by applying this formula:
S₁P₂ = S₂P₁
Making S₂ the subject of formula, we have:
S₂ = (S₁P₂)/P₁
S₂ = (0.42 × 3.0)/1.0
S₂ = 1.26 g/L.
Now, we can determine the mass:
Mass = solubility × volume
Mass = 1.26 × 1.00
Mass = 1.26 grams.
Read more on solubility here: brainly.com/question/3006391
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Answer:
235 g
Explanation:
From the question;
- Volume is 400.0 mL
- Molarity of a solution is 4.25 M
We need to determine the mass of the solute K₂CO₃,
we know that;
Molarity = Number of moles ÷ Volume
Therefore;
First we determine the number of moles of the solute;
Moles = Molarity × volume
Moles of K₂CO₃ = 4.25 M × 0.4 L
= 1.7 moles
Secondly, we determine the mass of K₂CO₃,
We know that;
Mass = Moles × Molar mass
Molar mass of K₂CO₃, is 138.205 g/mol
Therefore;
Mass = 1.7 moles × 138.205 g/mol
= 234.9485 g
= 235 g
Thus, the mass of K₂CO₃ needed is 235 g
Answer:
A snow leopard is one of the top consumers in the Himalayas who lives in dens that are close to somewhere to look down to watch its prey. They also use it's large paws to climb up slopes and snow and a long tale to balance on thin spaces to catch markhhors.
Explanation:
<h3>
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Answer:
The [H⁺] for this soluton is 2*10⁻³ M
Explanation:
pH, short for Hydrogen Potential and pOH, or OH potential, are parameters used to measure the degree of acidity or alkalinity of substances.
The values that compose them vary from 0 to 14 and the pH value can be directly related to that of pOH by means of:
pH + pOH= 14
In this case, pOH=11.30, so
pH + 11.30= 14
Solving:
pH= 14 - 11.30
pH= 2.7
Mathematically the pH is the negative logarithm of the molar concentration of the hydrogen or proton ions (H⁺) or hydronium ions (H₃O):
´pH= - log [H⁺] = -log [H₃O]
Being pH=2.7:
2.7= - log [H⁺]
[H⁺]= 10⁻² ⁷
[H⁺]=1.995*10⁻³ M≅ 2*10⁻³ M
<u><em>The [H⁺] for this soluton is 2*10⁻³ M</em></u>
