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### AuthorTopic: calculating molarity from pH  (Read 13205 times) !function(d,s,id){var js,fjs=d.getElementsByTagName(s)[0];if(!d.getElementById(id)){js=d.createElement(s);js.id=id;js.src="https://platform.twitter.com/widgets.js";fjs.parentNode.insertBefore(js,fjs);}}(document,"script","twitter-wjs"); (function() {var po = document.createElement("script"); po.type = "text/javascript"; po.async = true;po.src = "https://apis.google.com/js/plusone.js";var s = document.getElementsByTagName("script")[0]; s.parentNode.insertBefore(po, s);})();

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##### calculating molarity from pH
« on: April 24, 2005, 04:54:58 PM »

how do i get the molarity from pH?
the only quantative info i have to work with is: 75.0mL
(0.075 L) solution of "HCl", with a pH of 1.56.

my working is: [H+] = 10-pH = 10-1.56 = 2.75x10^-2M\L

But the question states: "From it's pH, calculate the molarity of HCl".

have I done this with my working or have I just gotten the hydrogen ion concentration ?

Any help or just a point in the right direction would be much appreciated.
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#### AWK

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##### Re:calculating molarity from pH
« Reply #1 on: April 24, 2005, 08:10:23 PM »

For strong acids a concentrationacid and the concentration of H+ are the same.
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#### Borek

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##### Re:calculating molarity from pH
« Reply #2 on: April 24, 2005, 11:54:13 PM »

For strong monoprotic acids, to be precise
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Chembuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info, pH-meter.info

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##### Re:calculating molarity from pH
« Reply #3 on: April 25, 2005, 03:40:06 PM »

Thanks alot for the quick response!!

hopefully i can return tha favour one day
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