Concentration: 2.5% w/v
Concentration w/v % = [mass of solute / volume of solution ] * 100
=> mass of solute = concentration w/v * volume of solution / 100
=> mass of solute = 2.5 * 750 ml / 100 = 18.75 grams
Also, using proportions you get to the same result:
2.5% w/v => 2.5 grams of NaOH / 100 ml of water
=> 2.5 grams of NaOH / 100 ml water = x grams of NaOH / 750 ml water
=> x grams of NaOH = 750 ml water * 2.5 grams of NaOH / 100 ml water
=> x = 18.75 grams of NaOH
Answer = 18.75 grams of NaOH
Answer:
The mass percentage of the solution is 10.46%.
The molality of the solution is 2.5403 mol/kg.
Explanation:
A bottle of wine contains 12.9% ethanol by volume.
This means that in 100 mL of solution 12.9 L of alcohol is present.
Volume of alcohol = v = 12.9 L
Mass of the ethanol = m
Density of the ethanol ,d= 
Mass of water = M
Volume of water ,V= 100 mL - 12.9 mL = 87.1 mL
Density of water = D=1.00 g/mL
Mass percent
Molality :
M = 87.1 g = 0.0871 kg (1 kg =1000 g)
HA and HB are present in concentrations of 0.182 M and 0.153 M, respectively.
<h3>What kind of acids are monoprotic?</h3>
Monoprotic acids include benzoic acid (C6H5CO2H), acetic acid (CH3CO2H or HOAc), nitric acid (HNO3), and hydrochloric acid (HCl).
<h3>How can you tell if a substance is monoprotic?</h3>
Any acid with only one hydrogen atom in its formula is called a monoprotic acid, while some acids with multiple hydrogen atoms may also fall under this category. In other words, while all monoprotic acids contain only one hydrogen, not all single-hydrogen acids are monoprotic.
<h3>Do monoprotic acids have a low acidity?</h3>
Because it easily loses its hydrogen ion in solution, the monoprotic acid HBr is regarded as being strong.
learn more about monoprotic acid here
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