We are being asked to determine the grams of the hydrochloride that must be dissolved in 10.00 mL of water to give a pH of 3.50
Thiamine hydrochloride (C12H18ON4SCl2) dissociates in water in the following manner
C12H18ON4SCl2 → C12H18ON4S2+ + 2 Cl-
Cl is neutral so it would not affect pH
C12H18ON4S2+ is a weak acid and it dissociates in water
C12H18ON4S2+ + H2O ⇌ HC12H18ON4S+ + H3O+
We are going to do the following steps
Step 1: Calculate [H3O+]
Step 2: Write Ka expression
Step 3: Determine [C12H18ON4S2+]
Step 4: Calculate mass of thiamine hydrochloride
Thiamine hydrochloride (C12H18ON4SCl2) is a water-soluble form of thiamine (vitamin B1; Ka = 3.37 x 10−7). How many grams of the thiamine hydrochloride must be dissolved in 10.00 mL of water to give a pH of 3.50?
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Based on our data, we think this problem is relevant for Professor Li & Thompson's class at PURDUE.
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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.