![]() ![]() Let's plug these numbers into the above equation: We know we have 10 g of HCl, which has a molecular weight of 36.5 g/mol. ![]() Let's do a quick example to help explain how to convert from moles to grams or grams to moles. If you wanted to find the concentration of the hydrochloric acid, you could use our concentration calculator. To know how to calculate moles, the equation is: It is, therefore, useful to find out exactly how many molecules of HCl are in the solution. Now, you want the resulting solution to be perfectly neutral, so you don't want to add too much or too little NaOH, making it too basic or acidic respectively. Let's say you want to neutralise 10 g of hydrochloric acid (HCl in water) with some sodium hydroxide (NaOH). So why do chemists use moles, and why do you need a mole calculator? Well, as we said above, it provides a useful metric when dealing with reactions. It turns out memorising that definition for my GCSE chemistry exam was pointless. Prior to that, a mole was defined as the number of atoms in 12 grams of carbon-12 (an isotope of carbon). ![]() The official International System of Units definition is that a mole is the amount of a chemical substance that contains exactly 6.02214076×10 23 ( Avogadro's constant) atoms, molecules, ions or electrons (constitutive particles), as of 20 th May 2019. A mole is how chemists define an amount of substance, useful when dealing with many different molecules reacting at once (i.e., any reaction). Just kidding – we're sure you've never heard that joke before. A mole is a small, subterranean mammal belonging to the family Talpidae. ![]()
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