Consider a buffer solution prepared from hocl and naocl. which is the net ionic equation for the reaction that occurs when naoh is added to this buffer? oh– + hocl → h2o + ocl– oh– + ocl– → hocl + o2– na+ + hocl → nacl + oh– h+ + hocl → h2 + ocl– 2 points save answer question 5
2 answers:
OH⁻ from strong base (NaOH) react with weak acid from buffer (HOCl) according to the following equation: OH ⁻ + HOCl → H₂O + OCl⁻
<u>Answer: </u> The ionic equation is written below.
<u>Explanation: </u>
We are given:
A buffer solution that is prepared from HClO and NaClO.
The given buffer solution is an acidic buffer because it is made up form a weak acid and its salt.
The component that neutralizes the additional hydroxide ions from sodium hydroxide in the solution is HClO
The ionic equation for the reaction that occurs when hydroxide ions are added follows:
Hence, the ionic equation is written above.
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Answer:
V¹N²= V²N²
here V¹= ?
N¹= 6.00
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So V¹= (V²N²)/N² = (175 x 0.2)/6
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