Question

In a sample of blood at 25°C, hydrogen ion concentration is 4.6x10^-8 M. Find the
concentration of OH ion and decide whether the sample is acidic, basic or neutral.​

Answer 1

Answer:

ph of very Dilute Solution is just

Less Than 7

ex - 6.98

Not need to solve Question

just see

{H+} < 10^-7

Answer 2

The hydroxide ion concentration in the solution is $2.19\times 10^{-7}M$ and the solution is basic in nature.

Explanation:

To calculate the pH of the solution, we use the equation:

$pH=-\log[H^+]$

We are given:

$[H^+]=4.6\times 10^{-8}M$

Putting values in above equation, we get:

$pH=-\log(4.6\times 10^{-8})\\\\pH=7.34$

To calculate the hydroxide ion concentration, we first calculate pOH of the solution, which is:

pH + pOH = 14

pOH = 14 - 7.34 = 6.66

To calculate pOH of the solution, we use the equation:

$pOH=-\log[OH^-]$

We are given:

pOH = 6.66

Putting values in above equation, we get:

$6.66=-\log[OH^-]$

$[OH^-]=10^{-6.66}=2.19\times 10^{-7}M$

There are three types of solution: acidic, basic and neutral

To determine the type of solution, we look at the pH values.

• The pH range of acidic solution is 0 to 6.9
• The pH range of basic solution is 7.1 to 14
• The pH of neutral solution is 7.

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