When a volume of 60.0 mL of 0.200 M HBr is mixed with a volume of 30.0 mL of 0.400 M CH3NH2, The pH value is mathematically given as
pH=10.64
<h3>What is
the pH value when 60.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH₃NH₂?</h3>
Question Parameters:
The pH when 60.0 mL of 0.200 M HBr
30.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 × 10^{-4}).
Generally, the equation for the Chemical Reaction is mathematically given as
H Br + H_3C NH_2----- > CH_3 NH_3 Br
Therefore
oH=p^{kb}+-log
OH=-log(4.4*10^{-4})+
OH=3.36
In conclusion, The equation pH value
pH+OH=14
Therefore
pH+=14-3.36
pH=10.64
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Answer:
Explanation:
There are 6.87 x 1023 atoms in 1.14 mol SO3, or sulfur trioxide (mol is the abbreviation for mole).
To determine the mass of sucrose from a given volume of solution, we need to convert the volume into mass by using the density of the solution. We calculate as follows:
mass solution = 3.50 ( 1118 ) = 3913 g
mass of sucrose = 3913 g solution ( .485 g sucrose / g solution ) = 1897.805 g sucrose is present in the solution.
Following reaction is involved in above system
HOCl(aq) ↔ H+(aq) + OCl-<span>(aq)
</span>OCl-(aq) + H2O(l) ↔ HOCl(aq) + OH-<span>(aq)
</span>
Now, if the system is obeys 1st order kinetics we have
K = [OCl-][H+<span>]/[HOCl] ............. (1)
</span>∴ [HOCl-] / [OCl-] = [H+] (1 / 3.0 * 10-8<span>) ............. (2)
</span>
and now considering that system is obeying 2nd order kinetics, we have
K = [OH-][HOCl-] / [OCl-] ................. (3<span>)
</span>Subs 2 in 3 we get
K = [OH-][H+] (1 / 3.0 * 10-8<span>)
</span>we know that, [OH-][H+] = 10<span>-14
</span>∴K = 3.3 * 10<span>-7
</span>
Thus, correct answer is e i.e none of these
