Problem #2: A generic weak acid, formula = HA, has a concentration of 0.200 M and is 1.235% dissociated. Ka of CH3NH2 is 2.27*10^-11. This colorless gas is a derivative of ammonia, but with one hydrogen atom being replaced by a methyl group. Ka = 10^-14/Kb = 2.72*10^-11. Determine the K a.. I looked … first, we must obtain the Ka (dissociation constant) for CH3NH2, which you can look up or derive. What is the pH of a 0.150 M solution of CH3COOH? a. What is Ka at 25 °C for the following equilibrium? Kb of CH3NH2 = 4.4 × 10−4. Source(s): https://shrink.im/ba1n0. The solution is acidic. Learning Strategies 1. Methylamine is a good nucleophile as it is an unhindered amine. 3 1. mcdannold. Kb Of Ch3nh2. The solution technique for this type of problem works for almost all weak acids. since Ka is small x will also be small, you can let O - x = O. x = [H+] = √[Ka*O] = 2.36*10^-6. Lv 4. Methylamine is an organic compound with a formula of CH3NH2. Gases; 2. Strong acids are listed at the top left hand corner of the table and have Ka values >1 2. 4 years ago. Chemistry 301. Kb(CH3NH2) = 4.4 × 10-4? i found it easiest to find the Kb value: Kb = 4.40 x 10-4 knowing that Kw = Ka x Kb, and that Kw = 1.0 x 10^-14, Ka = 2.27*10^-11. Thus the salt will be acidic. What is the value of Ka for the acid? 1.8 × 10-5. IMFs; 4. CH3NH2 is a weak base CH3NH3I is the salt of this weak base and a strong acid (HI). Thermo; FAQs; Links. Ka of HF = 3.5 × 10−4. Fundamentals; 1. I'm thinking this would be a weak base, and when I use Ka, I come up with pH of 8.2. Ka … Solution: Please note the use of a generic weak acid in the question. CH3NH3+(aq) + H2O(l) CH3NH2(aq) + H3O+(aq) Kb (CH3NH2) = 4.4 × 10–4 at 25 °C. Kb CH3NH2 = 3.7 x 10^4. 2.3 × 103 c. 4.4 × 10–10 d. 4.4 × 104 e. 2.3 × 10–11 Acid with values less than one are considered weak. As an amine it … But when I use Kb (which makes more sense to me) I come up with pH = 11.8. Ka CH3NH3+ = 2.7 x 10^-11. I completed a practice (not for marks) assignment for an organic chemistry course, and one of the questions asked for the pKa of methylamine. 0. 4.4 × 10–4 b. What is the value of Ka for the methylammonium ion, CH3NH3+? 5.68. Atomic; 3. Units . To determine the conjugate acid of CH3NH2 (methylamine), consider the acid-base reaction with water: CH3NH2 + H2O <> OH- + CH3NH3+ In the above reaction, methylamine accepts a proton from water and is thereby a Bronsted base. Plugging in the values found for the equilibrium concentration as found on the ICE table for the equation Ka = [H3O+][C2H3O2]/[HC2H3O2] allows the value of Ka to be solved in terms of x. 3. To find the Ka, solve for x by measuring out the equilibrium concentration of one of the products or reactants through laboratory techniques. 8.65. pH = 5.63. What is the pH of a 0.200 M CH3NH3Br solution? The strong bases are listed at the bottom right of the table and get weaker as we move to the top of the table. What is the pH of a 0.350 M MgF2 solution?
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