Question

In: Chemistry

Determine each of the following for a 0.170 M HBr solution: A.[H3O+] B.pH C.pOH D.Write the...

Determine each of the following for a 0.170 M HBr solution:

A.[H3O+]

B.pH

C.pOH

D.Write the balanced equation for the reaction with LiOH.

E. Calculate the volume, in milliliters, of HBr solution required to neutralize 46.0 mL of a 0.160 M LiOH solution .

Solutions

Expert Solution

(A) We have 0.170 M HBr solution. The dissociation of HBr is

So concentration of H+ ion, [] = 0.170 M

Also

Therefore the concentration of H3O+ , = 0.170 M

(B) pH of the HBr solution is,

(D) The reaction between HBr(acid) and LiOH(basic) results in LiBr(salt) and H2O balanced chemical equation of reaction between HBr and LiOH solution,

(E) We have the neutralization reaction,

We have the Molarity of HBr (M1) = 0.170M

Volume of the HBr solution (V1) =??

Molarity of LiBr solution (M2) = 0.160 M

Volume of LiBr solution (V2) = 46.0 mL

We can calculate the volume of HBr solution by using dilution law,

Volume of HBr requires to neutralise the LiOH solution,

V1 = 43.3 mL

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Determine each of the following for a 0.130 M HBr solution: a)Calculate the volume, in milliliters,...

Determine each of the following for a 0.130 M HBr solution: a)Calculate the volume, in milliliters, of HBr solution required to neutralize 46.0 mL of a 0.350 M LiOH solution . Acetic acid has a Ka of 1.8×10−5. b)What is the pH of a buffer solution containing 0.10 M HC2H3O2 (acetic acid) and 0.12 M C2H3O2−?

Determine the following in a 0.0390 M solution of HIO3 (Ka = 0.170)? [HIO3] = _____...

Determine the following in a 0.0390 M solution of HIO3 (Ka = 0.170)? [HIO3] = _____ M [IO31-] = _____M [H3O1+] = _____M pH = _____

Determine the volume of 0.170 M NaOH solution required to neutralize each sample of hydrochloric acid....

Determine the volume of 0.170 M NaOH solution required to neutralize each sample of hydrochloric acid. The neutralization reaction is: NaOH(aq) + HCl(aq)---->H2O(l)+ NaCl(aq) Part B 55 ml of a 0.065 M HCl solution Part C 155 ml of a 0.925 M HCl solution

25.0mL sample of 0.170 M CH3NH2with 0.145 MM HBr a) determine pH at equivalence point b)...

25.0mL sample of 0.170 M CH3NH2with 0.145 MM HBr a) determine pH at equivalence point b) determine the pHpH after adding 6.0 mLmL of acid beyond the equivalence point. given: Initial pH: 11.94 volume of added acid required to reach the equivalence point: 29.3 mL

A 360.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. A)...

A 360.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. A) What mass of NaOH could this buffer neutralize before the pH rises above 4.00? B) If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00? I keep getting 1.8 g and 3.5 g, which is wrong.

For each strong base solution, determine [H3O+], [OH−], pH, and pOH. A)8.89×10−3 M LiOH [OH−],[H3O+] =...

For each strong base solution, determine [H3O+], [OH−], pH, and pOH. A)8.89×10−3 M LiOH [OH−],[H3O+] = b)8.89×10−3 M LiOH pH,pOH= C)1.15×10−2 M Ba(OH)2 [OH−],[H3O+]= D)1.15×10−2 M Ba(OH)2 pH,pOH = E)1.8×10−4 M KOH [OH−],[H3O+]= F)1.8×10−4 M KOH pH,pOH = G)4.9×10−4 M Ca(OH)2 [OH−],[H3O+] = H)4.9×10−4 M Ca(OH)2 pH,pOH =

Determine pH for a solution containing 0.7 M HBr and 1.4 M HC3H5O2.

A 340.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. Part...

A 340.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. Part A What mass of NaOH could this buffer neutralize before the pH rises above 4.00? Express your answer using two significant figures. m = g Part B If the same volume of the buffer was 0.350 M in HF and 0.350 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00? Express your answer using two significant figures.

A 350.0 −mL buffer solution is 0.170 M in HFand 0.170 M in NaF. A) What...

A 350.0 −mL buffer solution is 0.170 M in HFand 0.170 M in NaF. A) What mass of NaOH could this buffer neutralize before the pHrises above 4.00? B) If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00?

Consider the titration of a 34.0 mL sample of 0.170 M HBr with 0.200 M KOH....

Consider the titration of a 34.0 mL sample of 0.170 M HBr with 0.200 M KOH. Determine each of the following: 1. initial pH 2. the volume of added base required to reach the equivalence point 3. pH at 10.4 mL of added base 4. pH at the equivalence point

Subjects