For acids, "weak" and "strong" have nothing to do with concentration. They're intrinsic properties of the specific acid. So that part of the question is unanswerable.
Whether it would be harmful or not also depends on the acid. Acetic acid at that concentration is very dilute vinegar. Prussic acid at that concentration is highly toxic.
If you concentrate a solution, the molarity (moles/liter) will increase.
would molarity increase, decrease, or stay the same if the room temperature increased by 5 degrees centigrade
molarity of moles of solute/liters of solution(not solvent) the volume of the solvent(even if it started at 1 L) would change after adding the solute depending on the molar mass, density, etc of the solute, the molarity would be different
There would be 117g of NaCl in 1000 ml or 1 liter. The MWt of NaCl is 58.5 so 117/58.5 is 2.00 - so the molarity is 2.00 moles per liter of NaCl
HNO3 is a strong acid, which means it dissociates completely. This means you don't have to set up an equilibrium scenario; you can just go with the given molarity as also being the concentration of hydrogen ions [H+]. So, pH = -log(0.00884), which is about 2.05.
The number of moles of solute dissolved in 1 L of a solution would be the molarity. As an example, if you had 2 moles of solute in 1 liter the molarity would be 2M.
molarity of 5% NaCl solution would be 1.25M.
If you concentrate a solution, the molarity (moles/liter) will increase.
would molarity increase, decrease, or stay the same if the room temperature increased by 5 degrees centigrade
Molarity
It most certainly would affect the molarity of oxalic acid. When you change the volume, i.e. dilute, you decrease the molarity. It is the number of moles that doesn't change.
molarity
it will increase the molarity of the acetic acid
Molarity
The concentration of a solution can be expressed in many ways. One of them is as the molarity of the solution. A solution with molarity equal to one has one mole of the solute dissolved in every liter of the solutions
The question, as worded, is a little ambiguous. Rather, the question you should be asking is “What is the molarity of a 125 ml aqueous solution containing 10.0g of acetone?” Acetone is roughly 58 grams per mole. Therefore, a 125 mil solution with 10 g of acetone would contain roughly 0.17 moles, and the molarity would be roughly 1.4See the Related Questions for more information about how to calculate the molarity of a solution
The UV index is ona scale of 0-10 (10 being the most harmful) Which means yes, 12 is harmful, so you would need a very strong sunscreen or a better choice would be to stay indoors.