Carbonate — technique

Dissolving carbon dioxide into a chilled liquid under pressure to add effervescent bubbles and a bright, acidic prickle.

The science

Carbon dioxide dissolves into liquid in proportion to its partial pressure (Henry's Law), and solubility rises sharply as temperature falls — cold water holds roughly twice the gas of warm. Once dissolved, some CO₂ reacts with water to form carbonic acid (CO₂ + H₂O ⇌ H₂CO₃), which lowers pH and reads on the palate as tartness. The tingle itself is largely trigeminal: the enzyme carbonic anhydrase on the tongue converts CO₂ back to carbonic acid at the surface, stimulating touch and pain nerves alongside the taste of sourness. Force carbonation pushes tank CO₂ into cold liquid under pressure; natural carbonation traps the gas from a small secondary fermentation of added priming sugar inside a sealed bottle.

What changes

Acidity↑ 40

Body↑ 45

Sweetness↓ 15

Aroma↑ 15

BeforeAfter

Live lab

Carbonation

Henry's law in a glass — set the pressure and temperature, watch how much fizz dissolves and why a warm soda gushes.

How it's carbonated

Applied CO2 pressure12 psi (gauge)

Liquid temperature4 °C

Dissolved CO₂

2.52 vol

By mass

4.9 g/L

If it warmed to 25°

36 psi

Still / frizzante

Soft sparkle

Lively (beer / soda zone)

High-carb / bottle-conditioned

Champagne / gusher risk

Lively (beer / soda zone) · 2.5 vol — Lagers, most sodas, sparkling cider — crisp, refreshing, clean bead.

Cold liquid is thirstier for CO2 At 0 °C water dissolves roughly twice the CO2 it holds at 25 °C for the same pressure. That is why breweries carbonate near freezing and why a cold bottle stays crisp while a warm one foams over — the gas simply won't stay in warm liquid.

Volumes: the universal fizz unit One 'volume' is the volume of CO2 gas (at 0 °C, 1 atm) dissolved per volume of drink — about 1.96 g/L. Beer runs 2.0–2.7, soda 3.5–4, and Champagne 5–6, which is why a cork holds back nearly 90 psi at room temperature.

Warm + shaken = gusher The dissolved CO2 doesn't change when you warm a sealed can, but the pressure it exerts climbs fast with temperature. Shaking adds thousands of tiny bubble nuclei; open it and the supersaturated gas escapes explosively along that new surface area.

Going flat is Henry's law in reverse Air holds almost no CO2 (~0.04%), so an open drink is wildly supersaturated. CO2 keeps leaving until the dissolved amount matches the trivial pressure above the liquid — reached faster when warm, agitated, or poured over rough surfaces like ice.

Two ways to make the fizz Force carbonation applies CO2 from a tank and lets Henry's law dissolve it — fast, exact, used for soda and kegged beer. Natural (bottle-conditioning) instead adds a measured dose of priming sugar to a sealed bottle; the yeast ferments it and the trapped CO2 dissolves in — roughly 4 g/L of sugar per volume. It's slower and less precise but builds the finer, more integrated bead of real Champagne and cask-conditioned ale. Over-prime and the same pressure that makes bubbles makes bottle bombs.

The ways

Force (tank)Push CO₂ in under pressure — fast, precise and repeatable.

Natural (priming)Add a little sugar and yeast in a sealed vessel; fermentation makes the fizz (Champagne, real ale).

Ratios & timing

Carbonation level2.4–4 volumes CO₂

Force-carb pressure at 3 °C30–45 psi

Bottle priming sugar6–8 g/L

Gear

CO₂ cylinder with pressure regulatorCarbonation cap or diffusion stoneWhipping/soda siphon with CO₂ chargersPressure-rated (PET or Champagne) bottlesCorny keg and kegerator or ice bath

Works on

Plain water and seltzerCocktails and highballsFruit juices and shrubsBeer and ciderKombucha and sparkling wineNovelty carbonated fruit (grapes, berries)

Watch out

Warm liquid holds far less gas and pressurizes the vessel dangerously — always chill near 3 °C before charging, and never exceed a bottle's rated pressure.