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What is the molarity of a solution with 0.2 moles of KOH in 100 mL of water?
Wiki User
∙ 12y ago
Molarity = moles of solute/Liters of solution
get moles KOH
6.31 grams KOH (1 mole KOH/56.108 grams)
= 0.11246 moles KOH
0.250 M KOH = 0.11246 moles KOH/XL
0.11246/0.250
= 0.4498 liters
= 450 milliliters
Wiki User
∙ 13y ago
Wiki User
∙ 12y agoMolarity = moles of solute/Liters of solution ( 200.0 ml = 0.200 Liters )
find moles
5 M KOH = moles KOH/0.200 Liters
= 1 mole KOH
1 mole KOH (56.108 grams/1 mole KOH)
= 56.108 grams needed
-----------------------------------( perhaps 60 grams to keep significant figures right? )
Wiki User
∙ 11y agoDo you mean pH? Need moles KOH first. Then molarity. Then pH.
0.10 grams KOH (1 mole KOH/ 56.106 grams) = 0.00179 moles KOH
Molarity = moles of solute/Liters of solution
Molarity = 0.00179 moles KOH/1.0 L
= 0.00179 M KOH
=================Now,
- log(0.00179 M KOH)
= 2.75
14 - 2.75
= 11.3 pH
-------------
( the H +, if that is what you meant, = 2.8 pH, as you can see above )
Wiki User
∙ 12y ago0.2 moles of KOH in 100 mL (= 0.100 L!) of water is 0.2 mol / 0.100 L = 2.0 mol/L = 2M KOH
Wiki User
∙ 10y agoThe answer to the question and its workings is as follows. 10.0g KOH/ 56.11g/mole =0.178 mole of KOH litres x 0.200 moles/litre =0.178 moles litres=0.891 mL=891
Wiki User
∙ 9y ago793 ml
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