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What volume of 0.10 m naoh can be prepared from 250 ml of 0.30 m naoh?
Wiki User
∙ 12y ago
10.0 ml of a solution of 6.0 molar NaOH contains (10.0/1000)(6.0) = 0.060 moles of NaOH. Call the number of milliliters needed to make a solution that is 0.30 molar with this amount of NaOH v. Then 0.060/v = 0.30, or v = 50 ml. Ideally, this solution should be made by putting the 6.0 molar solution into a volumetric container calibrated to 50 ml, then diluting with water to the mark for 50 ml. As an approximation, 50 - 10.0 = 40 ml of water can be added, but this may not give an exact match because 6.0 molar NaOH solution probably has a density considerably higher than 1.00 grams/ml, the density of water at standard temperature and pressure, while the density of 0.30 molar solution is substantially less but may still not be as low as 1.00. Therefore, adding a specified volume of water may not result in a total volume equal to the sum of the volume of water added plus the 10.0 ml originally specified.
Wiki User
∙ 13y ago
Wiki User
∙ 11y agoSimple equality.
(volume)(1.40 M NaOH) = (260 ml)(0.590 M NaOH)
V = 153.4/1.40 = 110 milliliters of 1.40M NaOH solution required,
This should be filled up to exactly 260 mL with pure water (about 150 mL)
Wiki User
∙ 12y agoM1v1=M2V2 V2=M1V1\M2 V2=(2.5)(1L)/0.33=7.58L
Wiki User
∙ 14y ago.75 L because you multiply the L of NaOH by the Molarity of NaOH the divide it by the Molarity given of NaOH to get the volume needed
Wiki User
∙ 12y ago0.083 L
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