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Chemistry
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11 Dec 2019

Fe3+, Ca2+, and Mg2+ ions are present in hard water. Given this fact, can you propose an explanation for "soap scum" deposits that are common in sinks and bathtubs with hard water?

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Reid Wolff
Reid WolffLv2
13 Dec 2019

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Related questions

Hard water contains Ca2+, Mg2+, and Fe2+, which interfere with the action of soap and leave an insoluble coating on the insides of containers and pipes when heated. Water softeners replace these ions with Na+. Keep in mind that charge balance must be maintained. (a) If 1500 L of hard water contains 0.020 M Ca2+ and 0.0040 M Mg2+, how many moles of Na+ is needed to replace these ions? (b) If the sodium is added to the water softener in the form of NaCl, how many grams of sodium chloride are needed?

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Since soap and detergent action is hindered by hard water, laundry formulations usually include water softeners-called builders-designed to remove hard water ions (especially Ca2+ and Mg2+) from the water. A common builder used in North America is sodium carbonate. Suppose that the hard water used to do laundry contains 75 ppm CaCO3 and 55 ppm MgCO3 (by mass).

What mass of Na2CO3 is required to remove 90.0% of these ions from 10.0 L of laundry water?

Answers on other posts that have been incorrect: 1.3g, 1.4g, .668g

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