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0.04 M KOH produces an OH- concentration of 0.04 M. Thus, the pOH is -log 0.04 = 1.4 and the pH will be 14 - 1.4 = 12.6
9
-log(1.0 X 10^-4 M KOH) = 4 14 - 4 = 10 pH KOH ----------------
9
-log(3.5 X 10^-4 M) = 3.4559 14 - 3.4559 = 10.5 pH
10.332
What volume(L) of 3M KOH solution can be perpared by diluting 0.5 L of %M KOH solution?
Molarity = moles of solute/Liters of solution get moles KOH 6.31 grams KOH (1 mole KOH/56.108 grams) = 0.11246 moles KOH 0.250 M KOH = 0.11246 moles KOH/XL 0.11246/0.250 = 0.4498 liters = 450 milliliters
Molarity = moles of solute/volume of solution 0.500 M KOH = moles KOH/125 ml 62.5 millimoles, or to answer the question precisely, 0.0625 moles KOH
Molarity is the concentration of a solution, defined as moles per unit volume. Where, Molarity = moles / volume In this case the molarity of the HCl solution is 0.03 M The pH of this is calculated by the equation below pH = - log [H+] Where [H+] is the concentration of hydrogen ions/ protons present in the solution. As HCl only contains one hydrogen ion per molecule then the concentation of [H+] is 0.03 M Then the equation can be calculated (the minus sign is very important!) pH = - log 0.03 pH = 1.52 To summarise, Molarity of 0.03 M HCl solution is 0.03 M pH of 0.03 M HCl solution is 1.52
If 1.8 L of water is added to 2.5 L of a 7.0 M KOH solution, what is the molarity of the new solution?
Molarity = moles of solute/Liters of solution ( 220.0 ml = 0.220 Liters ) 0.500 M KOH = moles KOH/0.220 Liters = 0.110 moles KOH (56.108 grams/1 mole KOH) = 6.17 grams solid KOH needed