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.
Concentration of NaOH = 0.025 M = 0.025 Moles per Litre of SolutionVolume of Solution required = 5.00LWe can say therefore that:Number of Moles of NaOH needed to prepare the solution= Concentration of NaOH * Volume of Solution requiredTherefore:Number of Moles of NaOH needed to prepare the solution= 0.025M * 5.00L= 0.125molesFrom this we can say that 0.125 moles of NaOH are needed to prepare a 5.00 L solution with a concentration of 0.025M of NaOH.
1 mole of NaOH contains 6.02 x 10^23 molecules So 0.2 moles of NaOH contains 6.02 x 10^23 divided by 5
In order to make 0.02 N NaOH from 0.2 N NaOH, one needs to dilute it by 10 x (10 fold). Depending on the volume of 0.02 N NaOH needed, that will determine the volume of 0.2 N used. For example, to make 100 ml of 0.02 N NaOH, you would dilute 10 mls of 0.2 N to 100 ml. This is seen in the following calculation: (x ml)(0.2 N NaOH) = (100 ml) (0.02 N NaOH) and x = 10 ml
-log(10^-4 M NaOH) = 4 14 - 4 = 10 pH NaOH -----------------------
we need 0.8gm NaoH and dissolved in 10 ml of water to make 2N solution of NaoH .
Concentration of NaOH = 0.025 M = 0.025 Moles per Litre of SolutionVolume of Solution required = 5.00LWe can say therefore that:Number of Moles of NaOH needed to prepare the solution= Concentration of NaOH * Volume of Solution requiredTherefore:Number of Moles of NaOH needed to prepare the solution= 0.025M * 5.00L= 0.125molesFrom this we can say that 0.125 moles of NaOH are needed to prepare a 5.00 L solution with a concentration of 0.025M of NaOH.
1 mole of NaOH contains 6.02 x 10^23 molecules So 0.2 moles of NaOH contains 6.02 x 10^23 divided by 5
In order to make 0.02 N NaOH from 0.2 N NaOH, one needs to dilute it by 10 x (10 fold). Depending on the volume of 0.02 N NaOH needed, that will determine the volume of 0.2 N used. For example, to make 100 ml of 0.02 N NaOH, you would dilute 10 mls of 0.2 N to 100 ml. This is seen in the following calculation: (x ml)(0.2 N NaOH) = (100 ml) (0.02 N NaOH) and x = 10 ml
-log(10^-4 M NaOH) = 4 14 - 4 = 10 pH NaOH -----------------------
Balanced equation first.NaOH + HCl -> NaCl + H2OAll one to one so a simple equality will do here.(X ml)(0.43 M NaOH) = (10 ml)(0.1 M HCl)0.43X = 1X = 2.3 milliliters NaOH needed--------------------------------------
we need 0.8gm NaoH and dissolved in 10 ml of water to make 2N solution of NaoH .
pH=10, so pOH=14-10=4 [OH]=10^-pOH [OH]=10^-4 [OH]=0.0001
NaoH HAVE 6.022(10)23 IN HALF DROP.
The formula mass of sodium hydroxide, NaOH is 23.0+16.0+1.0=40.0 Amount of NaOH in 25.0g sample = 0.625mol
Multiply the original amount by 1.10 .
First, you must find the amount of moles of NaOH, using the concentration and volume given. By lowercase m, I'm assuming you mean molality, or molals of solution, which is the equation:molality (m) = (moles of solute) / (total volume of solution (in liters))To solve for moles of NaOH, your solute, rearrange the equation by multiplying volume on both sides to get:moles solute = (molality)(total volume of solution)Next, just plug in the information you know, which is 500 mL for the total volume and 125 m for the molality.***Volume for concentration problems must be converted to liters, so remember that 1 L = 1000 mLmoles NaOH = (125 m)(0.500 L) = 62.5 molesFinally, convert this to grams by finding the molar mass of NaOH using the periodic table:22.99 + 16.00 + 1.008 = 39.998 g/mol62.5 moles (39.998 g) / (1 mol) =249.875 grams NaOH
10 joules per second = 10 watts