- Using The Table Of The Weak Base Below You Have Chosen Methylamine As Your Weak Base In The Buffer Solution You Have A 1 (153.11 KiB) Viewed 63 times
Save Answer A coffee-cup calorimeter contains 70 mL of water with an initial temperature of 24.9°C. An unknown sample with a mass of 6.259 grams was placed inside making the water temperature rise up to 25.5°C. The initial temperature of the metal was 86.4°C. (Water: density = 1g/mL; specific heat = 4.184 J/g-°C). 2. What is the specific heat (J/g-°C) of the unknown sample? (Write your answer in 2 decimal places without the unit).
Based on the table of specific heat, what is the identity of the sample in the previous problem? (Write your answer in CAPITAL LETTERS) Table 1: Specific Heats of Common Substances Substance Specific Heat Capacity, C (J/g.°C) Water (liquid) 4.184 Ice at 0°C 2.010 Steam at 100°C 1.996 Aluminum 0.902 Chromium 0.461 Lead 0.128 Magnesium 1.020 Mercury 0.140 Tin 0.213 Zinc 0.387
Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. Values of K for Some Common Weak Bases Conjugate Acid Name Formula K Ammonia Methylamine Ethylamine Aniline Pyridine NH3 CH3NH2 C2H5NH2 CHÚNH C5H5N NH4+ CH3NH3+ C2H5NH3+ CH3NH3+ C3H3NH+ 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 1. Compute the pOH of the buffer solution. (Write your answer in 2 decimal places).