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What is the pH of 0.1 M HBr?
-log(0.1 M) = 1 pH
What is the Ph of a 0.0030 M HBr solution in water?
pH = - log10[H+] so 2.52
A solution of HBr has H 2.1 x 10-6 What is the pH of this solution?
By definition pH = -log[H+], so pH = -log(4.9*10-4) = 3.31Only at 25oC: pOH = 14.00 - pH, so 14.00 - 3.31 = 10.69 = pOH
What is the pH of HBr in Bromine water?
It depends on the concentration but this would be pretty acidic - pH of 0 -1 .
A 25.00 mL sample of HBr is titrated with 0.150 M standardized sodium hydoxide solution the endpoint was reached when 18.80 mL of titrant had been added calculate the molar concentration of the HBr?
(25.00ml HBr)( Molarity ) = ( 18.80ml NaOH )( 0.150 M ) Molar concetration of HBr = 0.108 M
What is the pH of 0.1 M HBr?
-log(0.1 M) = 1 pH
What is the Ph of a 0.0030 M HBr solution in water?
pH = - log10[H+] so 2.52
How do you determine the pH of a solution of 1.5 m of HBr?
pH=-log[H+] pH-log(1.2x10^-3) pH=2.92 since the the pH plus the pOH is always equal 14 14-2.92=11.08 so the pOH is 11.08
A solution of HBr has H 2.1 x 10-6 What is the pH of this solution?
By definition pH = -log[H+], so pH = -log(4.9*10-4) = 3.31Only at 25oC: pOH = 14.00 - pH, so 14.00 - 3.31 = 10.69 = pOH
What is the pH of HBr in Bromine water?
It depends on the concentration but this would be pretty acidic - pH of 0 -1 .
A 25.00 mL sample of HBr is titrated with 0.150 M standardized sodium hydoxide solution the endpoint was reached when 18.80 mL of titrant had been added calculate the molar concentration of the HBr?
(25.00ml HBr)( Molarity ) = ( 18.80ml NaOH )( 0.150 M ) Molar concetration of HBr = 0.108 M
What volume of a 0.582 M solution of HBr is needed for a reaction that requires 36.3 g of HBr?
The answer is 770,9 mL solution.
A 20.0ml sample of 0.800 m Hbr solution is titrated with 0.800 m NaOH solution calculate the pH of the solution after these volumes of base are added 12.5 ml 18.7 ml 20.0 ml 29.5 ml and 34.2?
Looks as if you will need to calculate the pH of the final solution. The formula you need will be [H+] = 1 x 10-6 M.
What is the concentration of a HBr solution in 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?
Balanced equation. KOH + HBr -> KBr + H2O everything is one to one, so... Molarity = moles of solute/liters of solution ( change ml to liters ) 0.25 M KOH = moles KOH/0.015 liters = 0.00375 moles of KOH this is as many moles that you have of HBr, so... Molarity of HBr = 0.00375 moles/0.012 liters = a concentration of HBr that is 0.31 M
What is the pH of ammonium bromide?
The pH of ammonium bromide:ammonium bromide=NH4BrNH4+is the conjugateacidof the weak baseNH3. It is acidic.Br-is the anion of the strong acid,HBr. It is neutral.Which makes the solutionacidicwith a pH < 7.
How many grams in 4.23 m mol of HBr?
The answer is 0,3422 grams.
What is the concentration of a HBr if 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?
0.75 M
