How much of NaOH (in grams) is needed to prepare 546 mL of solution with a pH of 10.00 ?
To calculate the amount of NaOH needed to prepare the solution, we need additional information, specifically the concentration of NaOH in the solution. The pH alone is not sufficient to determine the amount of NaOH required. Could you please provide the concentration of NaOH?
To determine the amount of NaOH needed to prepare a solution with a pH of 10.00, you need to take into account the concentration of the NaOH solution you want to use. The molarity (M) of the NaOH will determine the amount of grams required to achieve the desired pH.
Here's the step-by-step process to calculate the amount of NaOH:
Step 1: Find the pOH value.
The pOH is the negative logarithm (base 10) of the hydroxide ion concentration (OH-) in the solution. Since the pH is 10.00, the pOH can be calculated as pOH = 14 - pH = 14 - 10.00 = 4.00.
Step 2: Convert pOH to OH- concentration.
To find the OH- concentration, we can use the equation:
OH- concentration = 10^(-pOH).
In this case, OH- concentration = 10^(-4.00).
Step 3: Calculate the amount of NaOH needed.
To obtain the amount of NaOH in moles, we need to multiply the OH- concentration by the volume of the solution in liters:
moles of NaOH = OH- concentration x volume of solution (in liters).
The volume is given as 546 mL, which needs to be converted to liters by dividing by 1000:
volume of solution = 546 mL รท 1000 = 0.546 L.
Finally, to convert moles of NaOH to grams, we need to multiply by the molar mass of NaOH, which is 40.00 g/mol.
So, the formula to calculate the amount of NaOH (in grams) is:
grams of NaOH = moles of NaOH x molar mass of NaOH.
By following these steps, you should be able to calculate the grams of NaOH needed.