Question

In: Chemistry

i mix 500ml of 0.250 M HCNO with 250ml of 0.333 M NaCNO. i then add...

i mix 500ml of 0.250 M HCNO with 250ml of 0.333 M NaCNO. i then add 25ml of 1.00 M NaOH. A) how many moles of CNO- are in the beaker before the reaction takes place. B) what is the limiting reactant for the neutralization reaction

Solutions

Expert Solution

A )

The question relates to ' common ion effect ' ( ie. the degree of dissociation of

a soluble electrolyte is supressed due to addition of a common ion ' ) . HCNO is

a weak acid with Ka = 3.5 x 10-4 hence its degree of dissociation ( ie. number of

moles of the acid dissociated out of one mole ) is calculated using Ostwald's dilution

law. Accordingly

= SQRT ( Ka / C ) , where represents degree of dissociation of the acid

..............& C = concentration in moles

calculated* as =( 0.250 x 500 ) / 750

....................... = 0.166 M

.......... So , = SQRT {( 3.5 x 10-4 ) / 0.166 }

........................= 0.0459 x 10-2

...................or, = 4.59 x 10-4 M

This represents concentrations of H+  ion & also NCO- ion yielded by ionization of

HCNO in solution , which is much much less than unity ( <<< 1.0 ) and is therefore

insignificant. However , the total [ NCO- ] = [ NCO- ]  produced by ionization of the salt

NaCNO + [ NCO- ]yielded by ionization of HCNO

NaCNO is a strong electrolyte and therefore gets completely ionized

The [ NaCNO] in 750 ml of solution is = (0.333 x 250 ) / 750

..............................................................= 0.111 M

therefore[ NCO- ]   ion produced...........= ( 0.111 + 4.59 x 10-4 ) / L

again since( 4.59 x 10-4 ) is <<< 1.0 , it can be ignored

& the total NCO- in 750 ml of solution = ( 0.111 x 750 ) /1000

................................................................= 8.325 x 10-2 moles  

B)

H+ has to partcipate in neutralization reaction with a base its concentration decides the

limiting reagent ,and a limiting reagent is one which gets consumed first, Therefore on addition of 25 ml of 1M NaOH solution HCNO should be considered as the limiting reagent.

...............................................................................................................................................

* strength or concentrations of HCNO ,& NaCNO are calculated using relation,

M1V1 = M2V2


Related Solutions

Consider the titration of 25.0 mL of 0.175 M cyanic acid, HCNO, with 0.250 M LiOH....
Consider the titration of 25.0 mL of 0.175 M cyanic acid, HCNO, with 0.250 M LiOH. The Ka of HCNO is 3.5 * 10^-4. What is the volume of LIOH required to reach the equivalence point? b. calculate the pH after the following volumes of LIOH have been added: a. 0mL b. 5.0 mL c. 8.75 mL d. 17.5 mL
add formal charges to each resonance form of HCNO below
add formal charges to each resonance form of HCNO below
A 280.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium...
A 280.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium acetate. For acetic acid, Ka=1.8×10−5. Part A)  What is the initial pH of this solution? Part B)  What is the pH after addition of 0.0150 mol of HCl? Part C)  What is the pH after addition of 0.0150 mol of NaOH?
A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate...
A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4.​
A 500 ml sample of 0.0040 M HCNO is titrated with 0.0020 M RbOH. Calculate the...
A 500 ml sample of 0.0040 M HCNO is titrated with 0.0020 M RbOH. Calculate the pH for the solution after the following additions of RbOH: 0 ml, 250 ml, 750 ml, 999 ml, 1000 ml, 1000 ml, 1001 ml, 1250 ml, 1500 ml.
Given 1.00 L of a solution that is 0.200 M HC3H5O2 and 0.250 M KC3H5O2, a.)...
Given 1.00 L of a solution that is 0.200 M HC3H5O2 and 0.250 M KC3H5O2, a.) What is the buffer capacity of the solution? That is, how many millimoles of strong acid or strong base can be added to the solution before any significant change in pH occur? b.) Over what pH range will this solution be an effective buffer?
Calculate the pH in the titration of 20 mL of 0.125 M HCL with 0.250 M...
Calculate the pH in the titration of 20 mL of 0.125 M HCL with 0.250 M NaOH solution after adding 9.60 mL and 10.40 mL of NaOH
Part A. Calculate the pH of a buffer solution that is 0.250 M in HCN and...
Part A. Calculate the pH of a buffer solution that is 0.250 M in HCN and 0.168 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). Part B. Calculate the pH of a buffer solution that is 0.240 M in HC2H3O2 and 0.190 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) Part C. Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate the pH of 1.0 L of...
A steel rod 0.450 m long and an aluminum rod 0.250 m long, both with the...
A steel rod 0.450 m long and an aluminum rod 0.250 m long, both with the same diameter, are placed end to end between rigid supports with no initial stress in the rods. The temperature of the rods is now raised by 60.0 ∘C. What is the stress in each rod? (Hint: The length of the combined rod remains the same, but the lengths of the individual rods do not.) Psteel,Paluminium = ?
If you start with 200 mL of a 0.250 M hypochlorous acid / 0.300 M potassium...
If you start with 200 mL of a 0.250 M hypochlorous acid / 0.300 M potassium hypochlorite buffer, (HClO/ KClO), and add 20.0 mL of a 0.400 M sodium hydroxide, NaOH, what will be the final pH of the solution? (For HClO, Ka = 3.0 x 10−8)
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT