Parts-per-million is a form of concentration that is confusing to some. It is often used for aqueous solutions at low concentrations because, as you state in your question, in dilute solutions the density of water has not been affected ie. is still 1.00 g/mL.
parts per million is defined as micrograms of solute per milliliter of solution. This doesn't inherently make sense since micrograms are on the millionths scale, but mL are on the thousandth scale, so it would seem to be millionth per thousandth--Not so! Since the 1.00 mL of water weighs 1.00 g, ug/mL converts, for dilute aqueous solutions, to ug/g, which now makes sense as parts per million. So, from the information given, the calculation is quite simple:
0.0036 g Cl * 10^6 ug/1 g = 3600 ug Cl
1.00 L * 1000 mL/1L = 1000 mL
Concentration of Cl- in solution in ppm:
3600 ug Cl- / 1000 mL = 3.6 ppm Cl-
molarity = moles of solute/liters of solution
We know the moles of solute: 0.875 moles of glucose. We can easily determine the liters of solution by using the mass of water given (1.5 kg) and the density of water (approximately 1 kg/L): they're, for all intents and purposes, equal (the approximation isn't large enough to be appreciable here, nor would the volume of the solution appreciably change since the solute is a solid that will <em>dissolve into </em>the solvent). So, we have 1.5 L of solution.
Now, we plug in what we have:
molarity = 0.875 moles of glucose/1.5 L of solution = 0.58 M glucose
The answer is provided to two significant figures since we're given the mass of water to two significant figures.
1. put a 2 in front of H on the H2O
2. put a 2 in front of KCL and KF
3. put a 2 in front of HCl
4. put a 2 in front of AgNO and 2 in front of Ag
5. put a 2 in front of HCl and 2 in front of H2O
I can write these out if you need me to
Answer:
B.
Explanation:
If we add more SO2 gas to the reaction chamber. To the left. The reaction would drive
backwards to re-establish equilibrium (more reactants made).