Equilibrium and acid/base chemistry (Modules 5 and 6) quiz

The forward reaction speeds up and the system shifts to favour the products

Net rate of reaction is zero; concentrations remain constant

The reverse reaction speeds up and the system shifts to favour the reactants

The equilibrium constant $K$ changes its value as the system responds

Shift the equilibrium to the left (towards fewer moles of gas)

Have no effect at all on the position because $K$ does not change

Shift equilibrium to the right (fewer moles of gas)

Decrease the value of the equilibrium constant $K$

Acid = electron-pair acceptor; base = electron-pair donor

Acid = proton donor; base = proton acceptor

Acid = $\mathrm{H}^+$ in water; base = $\mathrm{OH}^-$ in water

Acid = electron donor; base = electron acceptor

$0.10$

$13.0$

$7.0$

$1.0$

$\mathrm{CO}_3^{2-}$

$\mathrm{H}_2\mathrm{CO}_3$

$\mathrm{OH}^-$

$\mathrm{CO}_2$

A strong acid together with an equal molar concentration of a strong base

Only pure deionised water at a neutral pH of seven

A weak acid and its conjugate base (or weak base and its conjugate acid)

A neutral salt formed from a strong acid and a strong base

Less than $7$

Greater than $7$

Cannot be determined

Exactly $7$

Their acid and conjugate base forms have different colours, and the ratio depends on pH

They are strong acids that fully ionise completely in water at every value of the pH

They react irreversibly and permanently with any $\mathrm{H}^+$ ions present in the solution

They chemically neutralise the analyte being titrated and shift the equivalence point

Reactant-favoured

Product-favoured (essentially goes to completion)

At equilibrium with equal forward and reverse extents

Endothermic

Shifts the position of the equilibrium to the right so that it strongly favours the formation of the products

Increases the numerical value of the equilibrium constant $K$ at the given temperature

Speeds up both forward and reverse reactions equally; equilibrium is reached faster but $K$ is unchanged

Decreases the activation energy of only the forward reaction and leaves the reverse unchanged

Increase $K$ and shift equilibrium right

Have no effect on $K$

Always decrease the rate

Decrease $K$ and shift equilibrium left

Blood pH is held between $7.35$ and $7.45$ by the bicarbonate buffer system, with deviations producing acidosis or alkalosis that compromise enzyme function and oxygen transport.

Buffers are found everywhere throughout the human body, and they are very useful and important chemicals that help to keep many things working and stable in lots of different ways every single day.

In this extended response I am going to explain and describe in detail what blood pH is and why it matters.

Blood is a very important fluid in the human body and it does many things that are essential for survival.