(a)
Interpretation : The moles of
Concept Introduction : The mole concept is mainly used to determine the stoichiometry of any
(a)
Answer to Problem 1ASA
In the given reaction,
Explanation of Solution
Given:
Mass of
Formula mass of
Concentration of
Final volume of solution =
Substitute the values in the given formula to calculate no. of moles of
(b)
Interpretation : The molarity of
Concept Introduction : The mole concept is mainly used to determine the stoichiometry of any chemical reaction. It is used to calculate the mass of the reactant used or the amount of product formed during the chemical reaction. The relation between mass and moles of any chemical substance can be written as:
(b)
Answer to Problem 1ASA
In the given reaction the molarity of
Explanation of Solution
Given:
Mass of
Formula mass of
Concentration of
Final volume of solution =
Calculated the moles of
Expression for molarity is as follows:
Hence molarity of
(c)
Interpretation : The mole of
Concept Introduction : The mole concept is mainly used to determine the stoichiometry of any chemical reaction. It is used to calculate the mass of the reactant used or the amount of product formed during the chemical reaction. The relation between mass and moles of any chemical substance can be written as:
(c)
Answer to Problem 1ASA
In the given reaction mole of
Explanation of Solution
Given:
Molarity of
Volume =
Relation between molarity and volume is as follows:
Substitute values in the above expression to calculate no. of moles as follows:
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Chapter 28 Solutions
CHEMICAL PRIN.IN THE LAB-LM>CUSTOM<
- What volume of 0.10 moldm-3 sulphuric acid would be required to neutralise a mixture of 1.06 g of anhydrous sodium carbonate and 4.00 g of sodium hydroxide? (H2SO4 + 2NaOH ---> Na2SO4 + 2H2O) and (H2SO4 + Na2CO3 ® ---> Na2SO4+ H2O + CO2)arrow_forwardWhat mass of solid product is formed when 50.0 mL of 0.10 M Pb(NO3)2 (aq) is mixed with 75.0 mL of 0.10 M NaCl (aq)? Assume a 100% yield. Thank you!arrow_forwardWhat volume of 0.300 M H2SO4 can be made from 15.5 mL of 0.624 M H2SO4?arrow_forward
- Because of the toxicity of mercury compounds, mercury(I)chloride is used in antibacterial salves. The mercury(I) ion(Hg₂²⁺) consists of two bound Hg⁺ ions.(a) What is the empirical formula of mercury(I) chloride?(b) Calculate [Hg₂²⁺] in a saturated solution of mercury(I) chlo-ride (Ksp=1.5X10⁻¹⁸).(c) A seawater sample contains 0.20 lb of NaCl per gallon. Find[Hg₂²⁺] if the seawater is saturated with mercury(I) chloride.(d) How many grams of mercury(I) chloride are needed to satu-rate 4900 km³ of pure water (the volume of Lake Michigan)?(e) How many grams of mercury(I) chloride are needed to satu-rate 4900 km³ of seawater?arrow_forwardQuantity Your Data 1. Grams of vinegar sample used for your titration 25.000 g 2. Initial Buret Reading of Sodium Hydroxide solution 10.00 mL 3. Final Buret Reading of Sodium Hydroxide solution 28.00 mL 4. Amount of Sodium Hydroxide Solution used to neutralize the vinegar sample 5. Concentration of NaOH in the NaOH solution 0.050 g/mL 6. Grams of NaOH used to neutralize the vinegar 7. Grams of acetic neutralized by the amount of NaOH 8. Percent acetic acid in the vinegar Hints: For #4, The amount of NaOH used is the difference between the starting buret value and the ending buret value. For #6, Once you calculate the amount of sodium hydroxide used, multiple that value by the concentration of NaOH in the NaOH solution. For #7, Multiply the value obtained in number 6 by the number 1.5. Remember, we learned that every 1 gram of NaOH neutralizes 1.5 grams of acetic acid. For #8, Divide the grams of acetic acid by the grams of vinegar sample and multiply this value by…arrow_forwardWhat mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is added to 20.0 mL of 1.00 M NaBr?arrow_forward
- Try and answer the following questions without using a calculator. a A solution is made by mixing 1.0 L of 0.5 M NaCl and 0.5 L of 1.0 M CaCl2. Which ion is at the highest concentration in the solution? b Another solution is made by mixing 0.50 L of 1.0 M KBr and 0.50 L of 1.0 M K3PO4. What is the concentration of each ion in the solution?arrow_forwardcalculate weight of AgCl when added excess of AgNOs to 0.75g of BaCl2 if M.wt AgCl=143.3 and M.wt BaCk=208.3 AgNO3+ BaClz + BaNOsarrow_forward20. 50 ml of a 0.874 M HNO3 solution is diluted to 0.250 l. What is the concentration of the diluted solution ? a) 0.525 Mc) 0.350 M b) 0.175 M d) 4.37 Marrow_forward
- Answer the following questions regarding concentration: What concentration of ClO−3ClO3− results when 645 mL645 mL of 0.355 M AgClO30.355 M AgClO3 is mixed with 759 mL759 mL of 0.549 M Mn(ClO3)2? A 73.0 mL73.0 mL portion of a 1.30 M1.30 M solution is diluted to a total volume of 208 mL.208 mL. A 104 mL104 mL portion of that solution is diluted by adding 169 mL169 mL of water. What is the final concentration? Assume the volumes are additive.arrow_forward9. A 50.0 mL solution of acetic acid (CH3COOH) was titrated. In the process 35 mL of a 1.00 M NaOH standard were consumed. find the molarity of the acetic acid. If the density of the acetic acid solution is 1.08 g/mL, calculate the % acetic acid in the sample. CH3COOH + NaOH CH3COONa + H2Oarrow_forward5.00 mL of 2.32 M Fe(NO3)3 is combined with 1.00 mL of 0.50 M HClO4 and 4.00 mL of 2.00 × 10–2 M KSCN. What is the concentration of Fe3+ in the solution after the other reactants are added? Enter your answer with two decimal places. Example: 1.32arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning