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A US fluid ounce is 1 / 16 of a US pint (about 1·04 UK fluid ounces or 29.6 mL); a UK fluid ounce is 1 / 20 of a UK pint (about 0·96 US fluid ounce or 28.4 mL). On a larger scale, perhaps for institutional cookery, a UK gallon is 8 UK pints (160 UK fluid ounces; about 1·2 US gallons or 4.546 litres), whereas the US gallon is ...
The percentage is a mass concentration, so a 5% glucose/dextrose solution contains 50 g/L of glucose/dextrose (5 g per 100 ml). This usage is imprecise but widely used, as discussed at Mass concentration (chemistry) § Usage in biology. Glucose provides energy 4 kcal/gram, so a 5% glucose solution provides 0.2 kcal/ml.
For example, in a recipe that calls for 10 pounds of flour and 5 pounds of water, the corresponding baker's percentages are 100% for the flour and 50% for the water. Because these percentages are stated with respect to the weight of flour rather than with respect to the weight of all ingredients, the sum of these percentages always exceeds 100%.
To put this in context, most 12-US-fluid-ounce (355 ml) cans of soda contain 39 grams of sugar. In the United States, a government survey on food consumption in 2013–2014 reported that, for men and women aged 20 and older, the average total sugar intakes—naturally occurring in foods and added—were, respectively, 125 and 99 g/day. [153]
Many dry ingredients, such as granulated sugar, are not very compressible, so volume measures are consistent. Others, notably flour, are more variable. Others, notably flour, are more variable. For example, 1 cup of all-purpose flour sifted into a cup and leveled weighs about 100 grams (3½ oz), whereas 1 cup of all-purpose flour scooped from ...
Simple syrup (also known as sugar syrup, or bar syrup) is a basic sugar-and-water syrup. It is used by bartenders as a sweetener to make cocktails, and as a yeast feeding agent in ethanol fermentation. The ratio of sugar to water is 1:1 by volume for normal simple syrup, but can get up to 2:1 for rich simple syrup. [6]
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The term molality is formed in analogy to molarity which is the molar concentration of a solution. The earliest known use of the intensive property molality and of its adjectival unit, the now-deprecated molal, appears to have been published by G. N. Lewis and M. Randall in the 1923 publication of Thermodynamics and the Free Energies of Chemical Substances. [3]