In the chemical precipitation process, the hardness causing ions are converted from [blank] forms. Calcium and magnesium become [blank] as the pH increases.

Unlock all questions

This demo includes only 20 questions. Upgrade to access hundreds of questions, flashcards, exam simulations, and disable ads.

Full question bankExam simulationsFlashcards

From $25.99Unlock all

Prepare for the ADEQ Water Treatment Levels 1 and 2. Study with tailored questions, in-depth explanations, and interactive quizzes. Elevate your skills and ensure exam success!

Multiple Choice

In the chemical precipitation process, the hardness causing ions are converted from [blank] forms. Calcium and magnesium become [blank] as the pH increases.

Raising the pH in chemical precipitation makes hardness-causing ions shift from soluble forms to insoluble forms. In water, calcium and magnesium exist dissolved as Ca2+ and Mg2+. When lime or other alkalis are added, the higher concentration of hydroxide ions causes these ions to precipitate as insoluble hydroxides, Ca(OH)2 and Mg(OH)2, removing hardness from the water. This is the key mechanism behind lime-softening: converting dissolved hardness ions into solid precipitates as pH increases. (Carbonate precipitation can also occur in some systems, but the primary idea here is formation of insoluble hydroxides with rising pH.)

In the chemical precipitation process, the hardness causing ions are converted from [blank] forms. Calcium and magnesium become [blank] as the pH increases.

Prepare for the ADEQ Water Treatment Levels 1 and 2. Study with tailored questions, in-depth explanations, and interactive quizzes. Elevate your skills and ensure exam success!

In the chemical precipitation process, the hardness causing ions are converted from [blank] forms. Calcium and magnesium become [blank] as the pH increases.

Get the latest from Passetra