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What is an example of a buffer

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1. Where do water and hydrochloric acid (HCl) lie on the pH scale in relation to each other?

2. What is an example of a buffer, and describe what it is used for.

3. Why are conjugate pairs composed of weak acids and strong bases, and vice versa.

4. Showing work - Calculate the number of atoms of nitrogen contained in 162.5 g sodium azide, NaN3.

Write the equation g → mol → atoms

5. In the Haber process, used industrially to produce ammonia in massive tonnage, nitrogen reacts with hydrogen to form ammonia according to: N2 + 3H2 → 2NH3

What is the quantity (moles, grams) of ammonia produced upon the reaction of 1.70 mole nitrogen? Showing work

6. What is the mass (grams) of ammonia produced when 58.5 g hydrogen and 280 g nitrogen react to form ammonia? showing work

7. Precipitation reactions such as the subject of experiment one occur when the ions of a highly insoluble ionic compound are brought together in solution. These occurrences may be predicted according to empirical rules of solubility for common ionic compounds (attached below.)

a) Which of these rules predicts the identity of the precipitate formed in the mixture of solutions of calcium chloride and sodium carbonate?

b) Which of these rules predicts an identity for the precipitate formed when solutions of barium nitrate and sodium sulfate are mixed?

8. What is the balanced chemical for the double replacement reaction which occurs upon the mixing of solutions of sodium carbonate and calcium chloride. 

9. Calculate the molar mass of barium nitrate, and of sodium sulfate. showing work

10. Would there be any effect on an experiment if tap water containing calcium ions is used instead of deionized water to dissolve reactants?

Reference no: EM132252054

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