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pKa+pKb=pKw=14
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∙ 12y ago
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Place value: hundredsFace value: three hundred.Place value: hundredsFace value: three hundred.Place value: hundredsFace value: three hundred.Place value: hundredsFace value: three hundred.
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What is the pH if pKw is 14.26?
I will assume you are asking about the pH of pure water if pKw is 14.26. The relationship between pH, pOH, and pKw is as follows: pH + pOH = pKw. If it is pure, neutral water (no acids or bases present), then pH = pOH, so: pH + pOH = 14.26 2(pH) = 14.26 pH = pOH = 7.13
Where is Sam's Club on cobb pkw in marietta ga?
there is not
Is it true that the sum of pka and pkb is always equal to 14 at all temperature for any acid?
No it is not true because value of pkw changes with change of temperature. It's value is 14 at 250C and less at high temperature
How do you use pka to find the pH value?
PKa = -log Ka so if you multiply across by -1 and then taking the antilog you can get Ka Ka.Kb = Kw where Kw = 1.0 x 10^14 PKa + PKb = PKw = 14 that should give you a start.
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red car = rotes Auto red car = roter Wagen red car = roter PKW
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The address of the On The Chisholm Trail Association is: 1000 Chisholm Trail Pkw, Duncan, OK 73533-1539
Where can I find an industrial mixing equipment?
http://www.alfalaval.com/campaigns/tankequipment/mixing-and-agitation/product-overview/pages/product-overview.aspx?pkw=industrial%20mixing%20equipment is a website that you can find an industrial mixing equipment.
Calculate the pH of a 0.028 m NACN solution Ka 4.9 x 10 -10. the answer is 10.88 please help?
This is a weak base problem. Assume F = 0.028M Ka = 4.9 10^-10 Kb = Kw / Ka Kw - 10^-14 therefor pKw=14 x = [OH-] Kw / Ka = Kb = x^2 / (F-x) solve for "x" by use of quadratic formula to get the [OH-] pOH = -log [OH-] then plug pOH into the pH equation pH =pKw - pOH
How many times more hydroxide ions are there in a solution with a pH than in a solution with a pH of 3?
The concentration of hydroxide ion is realted to pH by the pKw (10-14) At pH 9 the concentration of OH- is 10-5, at pH 3, 10-11. The ratio is 106 so there are a million times as many OH- in pH 9.
How many more hydroxide ions are there in a solution with a pH of 9 than in a solution with a pH of 3?
The concentration of hydroxide ion is realted to pH by the pKw (10-14) At pH 9 the concentration of OH- is 10-5, at pH 3, 10-11. The ratio is 106 so there are a million times as many OH- in pH 9.
What is the pKw of water?
Here is the first step to convincing you that the pKa of water should not be 7: water is clearly a weaker acid than hydrogen sulfide, whose pKa is 7.04, or boric acid, 9.14, or hydrogen cyanide, 9.31 The real problem is why the pKa should not be 14.0 -- the same as pKw Here is the reason: Kw is defined as [H+]*[OH-], and this turns out to be 1.E-14. For any acid HA in water, though, Ka is defined as [H+]*[A-]/[HA] So if we think of water as an acid, Ka = [H+] * [OH-] / [H2O] = 1.0E-14 / [H2O] What do we do for [H2O]? Well, 1 g of water occupies 1 mL, near enough, which means that 18 gram of water = 1 mol of water occupies 18 mL. So we can fit 55.6 mol of pure water in 1.00 L. It is therefore fair to say that the "concentration" of water is 55.6 M, and so Ka = 1.8E-16 The log of 1.8E-16 to base 10 is -15.75, which is the pKa value quoted in your question.
How many times more hydroxide ions are in a solution with a pH of 9 than in a solution with a pH of 3?
The concentration of hydroxide ion is realted to pH by the pKw (10-14) At pH 9 the concentration of OH- is 10-5, at pH 3, 10-11. The ratio is 106 so there are a million times as many OH- in pH 9.
