Answer:
it is B because the other answers logically dont fit in
Answer:
We will use an acid-base indicator to see changes in colour depending on the pH
Explanation:
The pH changes during a titration, so you could use an acid-base indicator to follow the changes in pH.
A is wrong. An acid-base titration does not usually form a solid, and it would be impractical to isolate a solid with a funnel.
B is wrong. There are no changes in mass.
C is wrong. Any changes in temperature would be too small to measure precisely with an ordinary thermometer.
At room temperature, number of moles of distilled water is 1 x10^-7. Hope it cleared your doubt.
Answer:
Ka = ( About ) 5 x 10^ - 8
Explanation:
Let us first identify the dissociation equation for this weak acid,
HA ⇌ ( H+ ) + A¯
Knowing this, we can tell what the equilibrium expression is, respectively,
Ka = ( [ H+ ] [ A¯ ] ) / [ HA ]
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Now let us use the given pH 3.99 to calculate [ H+ ], knowing that pH = −log [H+],
3.99 = - log[H+],
[H+] = 10 ^ - 3.99,
[H+] = ( About ) 1 * 10^-4 M
Substitute known values into the equilibrium expression,
Ka = [( 1 x 10^ - 4 ) ( 1 x 10^ ¯4 )] / 0.199,
Ka = ( About ) 5 x 10^ - 8
The Hydrogen ion concentration of a pH 3.8 solution would be higher than that of a solution with a pH of 6.2. This is because since the pH scale measures the concentration of Hydrogen ions. We know that a pH range of less than 7 is considered acidic and greater than 7 is basic. If a solution is more acidic it would possess more hydrogen ions than if it weren't. In this case a pH value of 3.8 is more acidic than pH 6.2.
