[OH-][H+] = 10-14
[H+] = 10-14/0.01
[H+] = 1.0 × 10-12
pH = -log[H+]
pH = -log 1.0 × 10-12
pH = 12
pH=10 pOH= -log(.00010) pOH=4 pH+pOH=14 pH=14-4 pH=10
just take a 100ml from the 1N, pour it into a new beaker and complete that new beaker to 1L volume with distilled water... you're just diluting by a factor of 10.
That's 10 idiot.... Ask from me the chem master woahahahahahahah............
The pH of 0.1 N NaOH is 13.0. NaOH is the chemical compound known as sodium hydroxide. It is soluble in water, has a molar mass of 39.997 g/mol and boiling point of 2,530 degrees F.
0.0010M is 10-3 molar. pH is the negative logarathim to base 10 of this concentration, so the pH would be -log10 10-3 = 3
its pH value is 2.
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add 10 grams of NaoH into 1000 ml water, it will give you NaoH of 0.25N. As for making 1N solution you need to disolve 40 grams of NaoH into 1 litre water.
it goes back to normal
When just enough strong acid (e.g. HCl) is used to neutralize a strong base (NaOH), the pH should be neutral (pH = 7.0).
Prepared 0.5M succinic acid and 0.5 NaOH and adjusted pH to desired value
formula for neutralizatrion is volume of acid X normality of acid = volume of base X normality of base so (0.3)(3) should equal (4)(volume) which is .225L. However, Ca(OH)2 contains 2 moles of OH resulting division of total volume needed by 2. Thus, the answer becomes .1125L or 112.5ml.
1 millimolar = 0.001 M NaOH ( a base, remember ) - log(0.001 M NaOH) = 3 14 - 3 = 11 pH ----------
You dont - adding NaOH increases pH.
-log(10^-4 M NaOH) = 4 14 - 4 = 10 pH NaOH -----------------------
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As NaOH is a strong base I would not be surprised to see a 14 pH at least.
HCl : makes it acidic. it decreases the pH NaOH : makes it alkaline. it increases the pH
The pH value for this solution is 13.
Sodium hydroxide, NaOH, has a very high pH, so it can be used to raise the pH of some mixture that is too acidic.
Supposed the acid and base are both strong: pH of the acid is 0.0 and the pH of the base (hydroxide) is 14.0
A 0.01 M solution of NaOH has a pH =13
Quantity matters. If there is a lot of buffer (in terms of moles) and relatively little NaOH then the buffer will prevent any change in pH. If there is relatively more NaOH than buffer, then of course the pH will rise.
The amount of NaOH needed to raise the pH from 8 to 10 depends heavily on the conditions. The amount of NaOH needed will increase as the volume of the solution increases. Even more importantly, buffers can stabilize the pH significantly. If buffers are presently, the pH change will be much more gradual, and more NaOH will be required.