Question

1. Calculate the [H3O+] of a 1.93 M HBrO solution at 25 ºC.

please show work.

Answer #1

To do this, you need to show the reaction involved of the
hydrolisis of this compound, and you should take account of the Ka
of this acid, because HBrO is a medium strong acid, but it does not
dissociate completely in solution. The Ka reported is
2x10^{-9}. Now the reaction, along with the ICE chart to
calculate the H3O+ is:

r: HBrO + H_{2}O <-------->
H_{3}O^{+} + BrO^{-} Ka =
2x10^{-9}

i: 1.93 0 0

e: 1.93-x x x

Writting the expression for the equilibrium constant:

2x10^{-9} = x^{2} / 1.93-x

Ka is a very small value, so we can assume that x would be very
small too, and we can neglect the substract of 1.93-x to 1.93 only.
Solving for x:

2x10^{-9} * 1,93 = x^{2}

x = 6.21x10^{-5} M = [H_{3}O^{+}]

Hope this helps

Calculate the [H3O+] of a 1.99 M HBrO solution at 25 ºC.

Please show all steps.
If you titrate 25.00 mL of a 0.09797 M solution of HBrO, having
Ka = 2.8 x 10-9, with 0.05000 M Ba(OH)2
solution:
a) Calculate the number of mL of Ba(OH)2 solution
needed to reach the equivalence point.
b) Calculate the pH inititally, before any Ba(OH)2
solution is added.
c) Calculate the pH at halfway.
d) Calculate the pH at the equivalence point.

Part A Calculate [H3O+] in the following aqueous solution at 25
∘C: [OH−]= 4.3×10−4 M .
Part B Calculate [H3O+] in the following aqueous solution at 25
∘C: [OH−]= 1.6×10−12 M .
Part C Calculate [H3O+] in the following aqueous solution at 25
∘C: [OH−]= 3.0×10−2 M .

Calculate the [H3O+] of the following polyprotic acid solution:
0.310 M H3PO4 Calculate the pH of this solution Calculate the
[H3O+] and pH of the following polyprotic acid solution: 0.360 M
H2C2O4. Calculate the pH of this solution.

Calculate [H3O^-], [ClO4^-], and [OH^-] in an aqueous solution
that is 0.165 M in HClO4(aq) at 25 degree C.
[H^+]= ???? M
[ClO4^-]= ??? M
[OH^-]= ???? M
Is the solution acidic, basic or neutral?

1. A 0.735 M solution of a weak acid is 12.5% dissociated.
(a)Calculate the [H3O+], pH, [OH -], and pOH of the solution. (b)
calculate the ka of the acid

three sig figs please.
a) 0.19 M HCl
calculate [H3O+] , [OH-], and pH
b)1.5 x 10^ -2 M HNO3
calculate [H3O+] , [OH-], and pH
c) a solution that is 7.5×10−2 M in HBr and
1.9×10−2 M in HNO3
calculate [H3O+] , [OH-], and pH
d) a solution that is 0.780% HNO3
by mass (Assume a density of 1.01 g/mL for the
solution.)
calculate [H3O+] , [OH-], and pH

PLEASE SHOW WORK
4. Calculate the [H+], pH and percent dissociation of a solution
that is 0.50 M in HOCl and 0.60 M in NaOCl.
5. Calculate the [H+], pH and percent dissociation of a solution
that is 1.0 M in aniline (C6H5NH2) and 1.2 M in C6H5NH3Cl.
6. A solution contains 0.60 mol of NH4Cl and 0.30 mol of NH3 in
1.5 L. What is the pH if 0.070 mol of HCl is added to this
buffer?

Calculate the concentration of H3O(aq) ions present at
equilibrium in a solution that is prepared by mixing 100 mL of .35
M HCN and 200 mL of .15 M NaCN.
Kc= 6.2E-10 HCN(aq) + H2O <---> H3O(aq) + CN(aq) (this is
an equation from a previous question used for this question
also)
Please so all work! Thanks!

For each of the following solutions, calculate the pH, pOH,
[H3O+], and [OH-] at 25⁰C.
A solution of 0.047 M LiOH
A solution of 0.0011 M HNO3
A solution with a pH of 9.12
A solution of 0.010 M HClO3

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