30.0 mL of 0.10M HCI is mixed with 25ml, of 0.10M NaOH. What is the pH of the mi

Question

30.0 mL of 0.10M HCI is mixed with 25ml, of 0.10M NaOH. What is the pH of the mixture? 12.0 2.0 2.3 11.7 13 A 0.20 M solution of a weak acid has a pH of 2. What is the % dissociation? 1% 2% 4% 5% 12.5% The K_a for hypochlorous acid (HClO) is 3.5 times 10^8. What is the pH of a 1.50M solution? 11.3 5.1 4.3 3.6 1.8 What is the concentration of the A^2 ion in the 0.20M solution? 4.0 times 10^9 3.7 times 10^4 8.0 times 10^9 7.4 times 10^4 1.9 times 10^2 A weak acid HA has a K_a value of 5.0 times 10^4. What is the K for the following reaction? A + H_2 O OH + HA 2.0 times 10^4 5.0 times 10^11 5.0 times 10^12 2.0 times 10^11 1.0 times 10^14 Determine the K_sp of BaSO_4 if it has a solubility of 0.778mg/L. MM(BaSO_4) = 233.4g/mol 15 times 10^5 3.4 times 10^-7 1.1 times 10^11 4.0 times 10^11. 3.6 times 10^12 21 & 22: Use the following information for questions. A Weak acid (H_2A) has a K_a1 of 126x10^-6 and a K_a2 of 8.0x10^-9. What is the pH of a 0.20M solution? 4.13 4.13 4.5 5.6 2.1 3.3 Determine the solubility (in g/L) of AgBr in a 0.30M solution of NaBr. (K_sp(AgBr) = 5.0 times 10^-13 MM = 188g/mol) 12 times 10^-10 3.1 times 10^-10 13 times 10^-5 2.1 times 10^-5 3.3 times 10^-1 Mg(OH)_2 has a K_sp of 5.6 times 10^-12 What would be the pH of a saturated solution of this salt? 3.8 10.3 10.1 11.2 11.9

Explanation / Answer

Question 18.

First, balance the reaction

HCl + NaOH = H2O + NaCl

then

calculate moles of each species

mol of HCl = MV = 30*0.1 = 3 mmol of H+

mol of NaOH = MV = 25*0.10 = 2.5 mmol of OH-

so

mmol of H+ left = 3-2.5 = 0.5 mmol of H+

recalcualte H+

Vtotal = 30+25 = 55 mL

[H+] = 0.5 mmol / 55 mL = 0.00909090 M

pH = -log(0.00909090) = 2.04

best answer is 2.0

Choose B

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