Quick questions on Simpler equilibria and acid-base reactions - WJEC A-Level Chemistry

In the Bronsted-Lowry model, every acid has a conjugate base formed when it loses a proton, and every base has a conjugate acid formed when it gains one. In the reaction $\text{HCl} + \text{H}_2\text{O} \rightleftharpoons \text{H}_3\text{O}^+ + \text{Cl}^-$, $\text{HCl}$ and $\text{Cl}^-$ are one conjugate pair and $\text{H}_2\text{O}$ and $\text{H}_3\text{O}^+$ are the other. Identifying these pairs makes clear that an acid-base reaction is simply a proton transfer, and that water can act as either an acid or a base depending on its partner.

Ammonia synthesis is run at a compromise of about $450$ degrees C and $200$ atm: high pressure favours the product side (fewer gas moles), while moderate temperature balances yield against rate, a direct application of Le Chatelier. Titration in the lab. The titration calculation above is the workhorse of standardising solutions and analysing unknown concentrations throughout the course.

Define a Bronsted-Lowry base. [1 mark]

State the effect of increasing temperature on an exothermic equilibrium. [1 mark]

Calculate the moles of hydrochloric acid in $20.0$ cm$^3$ of $0.150$ mol dm$^{-3}$ solution. [1 mark]

Identify the conjugate base of the acid $\text{HCl}$. [1 mark]

Explain the difference between a strong acid and a concentrated acid. [1 mark]