Soal Asam-basa Untuk Kelas Xi IPA

According to the Bronsted-Lowry theory, a base is defined as a substance that accepts a proton. In other words, it is a proton acceptor. This definition is different from the Arrhenius theory, which defines a base as a substance that produces hydroxide ions in water. Therefore, the correct answer is d. Akseptor proton.

According to Arhenius, an acid is a substance that can release H+ ions in water.

The correct answer is b. Asam klorida, asam sulfat, asam nitrat. These three compounds are strong acids because they completely dissociate in water, releasing a high concentration of hydrogen ions (H+). Asam klorida (HCl) is a strong acid commonly found in stomach acid. Asam sulfat (H2SO4) is a strong acid used in various industrial processes. Asam nitrat (HNO3) is a strong acid used in the production of fertilizers and explosives. These acids have a low pH and are highly corrosive.

The pH of a solution is a measure of its acidity or alkalinity. In this case, the solution is sulfuric acid (H2SO4) with a concentration of 0.005 M. Sulfuric acid is a strong acid that dissociates completely in water, producing hydronium ions (H3O+). The concentration of hydronium ions in a solution determines its pH. Since the concentration of hydronium ions in this solution is relatively high, the pH will be low. A pH of 2 indicates a highly acidic solution.

Menurut teori Lewis, asam adalah zat yang mampu menerima pasangan elektron dari zat lain. Sebagai akseptor pasangan elektron, asam akan membentuk ikatan kovalen dengan zat yang menyumbangkan pasangan elektron. Dalam hal ini, asam bertindak sebagai penerima elektron, sehingga menjadikannya jawaban yang tepat.

The given question asks for the pH of a solution containing 6 grams of acetic acid in 250 ml. To find the pH, we need to calculate the concentration of H+ ions in the solution. Acetic acid is a weak acid, so we can use the equation Ka = [H+][A-]/[HA] to find the concentration of H+. Since the concentration of acetic acid is given in grams, we need to convert it to moles by dividing by the molar mass. The molar mass of acetic acid is 60 g/mol. After finding the concentration of H+, we can use the formula pH = -log[H+] to calculate the pH. The final answer is 3 - log 2.

The given information states that the concentration of OH- in the solution is 1.10-4. The pH of a solution can be determined by taking the negative logarithm of the concentration of H+ ions. Since OH- and H+ ions are inversely related, we can use the equation pH + pOH = 14. By substituting the given concentration of OH- into the equation, we can find the pOH, which is 4. Therefore, the pH of the solution is 14 - 4 = 10.

The given correct answer is e. Dapat menetralkan larutan kalium amoniak. This statement suggests that the substance is able to neutralize a solution of potassium ammonia. However, a base is typically defined as a substance that can donate hydroxide ions (OH-) or accept protons (H+). The ability to neutralize a specific solution does not necessarily indicate a substance's basic properties.

When NaOH is dissolved in water, it dissociates into Na+ and OH- ions. Since NaOH is a strong base, it completely ionizes in water. As a result, the concentration of OH- ions in the solution increases, leading to a higher pH value. A pH of 13 indicates that the solution is highly basic.

The given question is asking for the pH of a 0.1 M solution of HCOOH (formic acid) with an ionization degree (α) of 0.01. The ionization degree (α) represents the fraction of the acid molecules that dissociate into ions in solution. Since HCOOH is a weak acid, it does not fully dissociate in water. The pH of a weak acid solution can be calculated using the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions. In this case, since the ionization degree is 0.01, the concentration of hydrogen ions ([H+]) is 0.01 times the initial concentration of the acid (0.1 M). Taking the negative logarithm of 0.01 * 0.1 gives a pH value of 2. Therefore, the correct answer is b. 3.