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Conversion

Water Hardness Unit Converter (gpg ↔ ppm ↔ mmol/L ↔ °dH)

Water hardness is the total amount of dissolved calcium and magnesium ions, reported in different units around the world. North America uses gpg and ppm CaCO₃, continental Europe uses German °dH and French °fH, and the UK traditionally uses English Clark °eH. This tool converts between all six at once and classifies the water as soft, moderately hard, hard or very hard per WHO/USGS bands. Useful for baristas, aquarists, softener installers and laboratory work.

Classification

Hard

120–180 mg/L CaCO₃ — scale forms in kettles and dishwashers; consider an ion-exchange softener.

Equivalent in other units

ppm (mg/L CaCO₃)
150.0
gpg (US grain / gallon)
8.8
mmol/L (CaCO₃ equivalent)
1.50
°dH (German degrees)
8.4
°fH (French degrees)
15.0
°eH (English / Clark degrees)
10.5

Formula

All conversions pass through ppm CaCO₃ (mg/L) as the canonical unit. 1 gpg = 17.118 ppm 1 °dH = 17.848 ppm 1 °fH = 10 ppm 1 °eH = 14.254 ppm 1 mmol/L CaCO₃ = 100.087 ppm

Frequently asked

Is hard water bad for health?

Generally not — and some research even suggests a small benefit. WHO (2011) reviewed multiple epidemiological studies and concluded: (1) hard water does not increase risk of kidney stones, cardiovascular disease or kidney disease. In fact, calcium and magnesium in drinking water can supply 5–20 % of daily intake, especially valuable for low-dairy diets. (2) Some case-control studies link hard-water regions to lower cardiovascular mortality, possibly via magnesium intake. (3) Conversely, very soft water (< 30 mg/L) can dissolve lead or copper from older plumbing — that's why parts of Scotland adjusted water-treatment policy in the 2000s. Hard water does cause genuine household nuisance though: kettle scale, soap-scum on clothes, dry-feeling skin (subjective), shorter coffee-machine life. Household softeners therefore solve convenience and appliance-protection problems, not health problems. One caution: ion-exchange softeners replace Ca²⁺/Mg²⁺ with Na⁺, slightly raising sodium content — people with kidney disease or hypertension should drink un-softened water at the tap.

Some labs report hardness as mg/L Ca²⁺ — how does that relate to ppm CaCO₃?

Both are mg/L but the denominator differs, so they don't interchange directly. The conversion uses the molar-mass ratio: M(CaCO₃) = 100.087 g/mol, M(Ca²⁺) = 40.078 g/mol. So 1 mg/L Ca²⁺ = (100.087 / 40.078) ≈ 2.497 mg/L CaCO₃. Example: a lab report of "Ca 40 mg/L, Mg 12 mg/L" gives hardness (as CaCO₃) = 40 × 2.497 + 12 × (100.087 / 24.305) = 99.9 + 49.4 ≈ 149.3 mg/L CaCO₃ — hard water. Similarly, a report "as CaO" multiplies by 100.087 / 56.077 ≈ 1.785 to convert to CaCO₃. Before entering a number, check whether it is on the CaCO₃ scale; if not, convert first using the ratios above.

How does scale in coffee machines relate to water hardness, and what is ideal?

There's a direct relationship, modulated by how much of the hardness is "temporary" (carbonate-bound). Scale is mostly calcium carbonate, deposited when temporary hardness is heated. If your water is mostly "permanent" hardness (sulphates or chlorides), heating produces less scale but still affects taste and crema. The Specialty Coffee Association (SCA, 2009) targets total hardness 50–175 mg/L CaCO₃ (ideal 75–125) and carbonate hardness 40–75 mg/L. London cafés (~300 mg/L) typically install RO + remineralisation to dial water into that range. Hong Kong tap (50–80 mg/L) sits at the lower end of the SCA window — usable, though espresso machines benefit from a small remineralisation salt boost. Order-of-magnitude check: 100 mg/L water heated to boiling deposits ~0.05 g of calcium salts per litre. A high-volume machine doing 100 cups/day (≈ 10 L) accumulates ~30 g of scale per month — explaining why regular descaling is essential. Softening or RO filtration is the durable fix; simply boiling water is not.

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