We hope this grams-to-moles calculator (or moles-to-grams calculator) will help you with your chemical calculations! You may also find our titration calculator useful. So we now know we need 10.8 g of NaOH to exactly neutralize our amount of hydrochloric acid. Mole × molecular weight = mass (rearrange the equation),Īs 1.626×10 23 molecules of NaOH is also equal to 0.27 moles, and we know that the molecular weight of NaOH is 40, we can use these numbers to get: Mole = mass / molecular weight (multiply both sides by molecular weight), As we need to find the mass of NaOH to add, let's quickly rearrange the equation: Now we know the number of molecules of HCl we have, and since the reaction is 1:1, we need the exact same number of molecules of NaOH to neutralize it. We can work out the number of molecules by multiplying the moles by Avogadro's constant above. 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. Then you multiply that by your 878 grams. You divide and find that 1 gram of fluorine is equal to 0.0525350025878 moles. If you take your 878 grams of fluorine and then look at the atomic mass. First you must covert your grams to moles, then you can take the moles and covert to atoms. To know how to calculate moles, the equation is: You cannot directly convert grams to atoms. 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. Start a second calculation using steps 1-6.A mole is a small, subterranean mammal belonging to the family Talpidae. The output from your first calculation to
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