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20.00mL of 0.55M CH3COOH solution

20.00mL of 0.55M CH3COOH solution is mixed with 9.95mL of 1.0M NaHCO3 solution.The reaction occurring is CH3COOH + NaHCO3 -->
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2. asked by Kate
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What is the molarity of the final solution of 2.00mL of the 5.00M stock solution is diluted to 10.00mL to make solution A.
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2. asked by jamie
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What is the molarity of the final solution if 2.00mL of the 5.00 M stock solution is diluted to 10.00mL to make solution A?
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2. asked by Chem
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In Chemistry: what is ph during the titration of 20.00ml of 0.1000m triethylamine (ch3ch2)3n (kb=5.2x 10-4) with 0.1000m HCL
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2. asked by jain
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10.0 mL of a 0.300M NH3 solution is titrated with a 0.100M HCl solution. Calculate the pH after the following additions of HCl.0
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2. asked by Raven
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9.00mL of 1.10M CH3COOH and 1.00mL of 0.900M CH3COO- what is the pH?
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2. asked by Reen
3. 720 views
The following two solutions were combined and mixed well: 150.00 mL of a 3.500 M iron(¡¡¡) nitrate solution and 760.00mL of a
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2. asked by Mantsha
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The following two solutions were combined and mixed well: 150.00 mL of a 3.500 M iron(¡¡¡) nitrate solution and 760.00mL of a
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2. asked by Anonymous
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What is the molar concentration of 4% (w/v) CH3COOH? Hence calculate the expected titre of 0.1M NaOH solution when reacting with
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2. asked by Stae
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The titration of 25.00mL of Ba(OH)2 solution with an aqueous solution of 0.500 M HCl reaches an end point when 30.20 mL of the
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2. asked by LISA
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