What will happen if a small amount of hydrochloric acid. HCI. is added to a 0.1

Question

What will happen if a small amount of hydrochloric acid. HCI. is added to a 0.1 M solution of HF? The percent ionization of HF will increase. The percent ionization of HF will decrease. k_a for HF will increase. k_a for HF will decrease. Ammonia, NH_3, is in a solution with dissolved ammonium nitrate, NH_4NO_3. If external NaOH is added, which ion will react with the extra hydroxide ions (OH^+) to keep the pH from changing? H^+ NH_3^- NO_3 NM^+_4 3. Which of the following(s) is false for a buffered solution? The solution tends to resist the change in ([H^+] when external acid or based is added. The solution can resist change in its [H^+] whether a huge amount of acid or base is added. The solution will not change its pH very much even if a small amount of strong base is added. The solution will not change its pH very much even if a small amount of strong acid is added. Which of the following mixtures would result in a buffered solution? Mixing 50.0 mL 0.100 M HCI with 100.0 mL of 0.100 M NH_3 (k_b = 1.8 times 10^-5). Mixing 100.0 mL of 0.100 M HCI with 100.0 mL of 0.100 M NaOH. Mixing 100.0 mL of 0.100 M HCI (K_B = 1.8 TIMES 10^-5) with 100.0 mL of 0.100 M NaOH. Mixing 100.0 mL of 0.100 M HCI with 100.0 mL of 0.100 M HCI (k_b = 1.8 times 10^-5). Suppose a buffer solution is made from chlorous acid (HCIO_2) and sodium chlorite (NaCIO_2), What is the next ionic equation for the reaction that occurs when a small amount of sodium hydroxide (NaOH) is added to this buffer? What combination of substances will give a buffered solution that has a pH of 5.05? K_b(NH_3) = 1.8 times 10^-5; k_b(C_5H_5N) = 1.7 times 10^-9 0.2 M NH_3 and 0.3 M NH_4Cl 0.2 M C_5H_5N and 0.3 M C_5H_5NHCI 0.3 M C_5H_5N and 0.2 M C_5HD_5NHCI A solution contains 0.250 M HA (k_a = 1.0 times 10^-6) and 0.45 M NaA. What is the pH after 0.27 mole of HCI(g) is added to 1.00 L of this solution? 0.57 7.54 5.54 2.07 8. In titrating 0.20 M HCI with 0.20 M NaOH at 25 degree C, the solution at the equivalence point is 0.20 M NaCI very acidic slightly basic 0.10 M NaCI 9. Consider the titration of 300.0 mL of 0.700 M NaOH_3 (k_b = 1.8 times 10^-5) with 0.300 M HNO_3. How many milliliters of 0.300 M HNO_3 are required to reach the equivalence point? 350.0 ml, 400.0 ml 700.0 ml 300.0 ml

Explanation / Answer

1) answer is b.

HF is a weak acid that only partially dissociates An equilibrium is establised in the HF solution
HF H+ + F-
If you then add some HCl to this solution you introduce a higher concentration of H+ ions . In order to restore the Ka for HF, the equilibrium moves to the left , the dissociation of the HF is reduced.

Ka = [H+] [F-] / [HF]
If you add H+ ions from HCl - the [H+] in soltion increases - therefore the [F-] has to reduce in order to maintain the Ka value . The dissociation of HF is reduced.

2) OH- reacts with the ammoni and produce NH2OH. so answer is B

3) A buffer solution (more precisely, pH buffer or hydrogen ion buffer) is an aqueous solution consisting of a mixture of a weak acidand its conjugate base, or vice versa. Its pH changes very little when a small amount of strong acid or base is added to it.

so ans is a.

4) ans is a.

all other option s are just neautralization reactions.

5) is b

If a strong base is added to a buffer, the weak acid will give up its H+ in order to transform the base (OH-) into water (H2O) and the conjugate base: HA + OH- A- + H2O. Since the added OH- is consumed by this reaction, the pH will change only slightly.

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.