what volume of dry hydrogen chloride gas at s.t.p will dissolve in 250cm^3 of water to produce a 0.05M solution of water
So what... Is dis a solution or not
Cause I need those answers ASAP
To calculate the volume of dry hydrogen chloride (HCl) gas at standard temperature and pressure (STP) that will dissolve in 250 cm^3 of water to produce a 0.05 M solution, we need to use the concept of molarity and the ideal gas law.
To begin, we need to convert the volume of water from cm^3 to liters. We divide 250 cm^3 by 1000 to obtain the volume in liters:
Volume of water = 250 cm^3 ÷ 1000 = 0.25 L
Next, we need to determine the number of moles of HCl required to make a 0.05 M solution using the formula:
Molarity (M) = Moles (mol) / Volume (L)
Rearranging the formula, we can solve for moles:
Moles (mol) = Molarity (M) x Volume (L)
Substituting the given values into the formula:
Moles of HCl = 0.05 mol/L x 0.25 L = 0.0125 mol
Now, we can use the ideal gas law to calculate the volume of dry HCl gas at STP. The ideal gas law states:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (STP is 273.15 K)
Rearranging the formula to solve for volume (V):
V = nRT / P
Substituting the given values:
V = (0.0125 mol) x (0.0821 L·atm/(mol·K)) x (273.15 K) / (1 atm)
V ≈ 0.277 L or 277 cm^3
Therefore, the volume of dry hydrogen chloride gas at STP needed to dissolve in 250 cm^3 of water to produce a 0.05 M solution is approximately 277 cm^3.
To find the volume of dry hydrogen chloride (HCl) gas that will dissolve in water to produce a 0.05 M (molar) solution, we can use the equation:
M1V1 = M2V2
Where:
M1 = initial molarity of the gas (unknown)
V1 = initial volume of the gas (unknown)
M2 = final molarity of the solution (0.05 M, given)
V2 = final volume of the solution (250 cm^3, given)
First, let's convert the volume from cm^3 to liters, since the molarity is usually expressed in moles per liter.
250 cm^3 = 250/1000 = 0.25 L
Now we can rearrange the equation to solve for V1:
V1 = (M2 * V2) / M1
Since we want to know the volume of the gas at STP (Standard Temperature and Pressure), we assume that the final volume (V2) of the solution also corresponds to this condition. At STP, one mole of any ideal gas occupies 22.4 L. So, we need to convert our final volume from L to moles of HCl:
V2 = 0.25 L / 22.4 L/mol = 0.01116 mol
Now, let's substitute the known values back into the equation:
0.01116 mol = (0.05 mol/L * V1) / M1
We still don't know the value of M1 (initial molarity of HCl gas), so we need to assume a value as a starting point. Let's assume M1 = 1 M, which is a standard concentration for many solutions.
0.01116 mol = (0.05 mol/L * V1) / 1 M
Simplifying the equation, we can solve for V1:
V1 = (0.01116 mol * 1 M) / 0.05 mol/L = 0.2232 L
Finally, let's convert the volume of the gas back to cm^3:
V1 = 0.2232 L * 1000 cm^3/L = 223.2 cm^3
Therefore, approximately 223.2 cm^3 of dry HCl gas at STP will dissolve in 250 cm^3 of water to produce a 0.05 M solution.
M = moles/L soln
0.05 = moles/0.250L
moles = 0.05 x 0.250 = 0.0125 moles HCl
Then moles x 22.4 = ?L HCl.