(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 Principles in the Laboratory
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- What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?arrow_forwardA 0.500-L sample of H2SO4 solution was analyzed by taking a 100.0-mL aliquot and adding 50.0 mL of 0.213 M NaOH. After the reaction occurred, an excess of OH ions remained in the solution. The excess base required 13.21 mL of 0.103 M HCl for neutralization. Calculate the molarity of the original sample of H2SO4. Sulfuric acid has two acidic hydrogens.arrow_forwardSuppose you dilute 25.0 mL of a 0.110 M solution of Na2CO3 to exactly 100.0 mL. You then take exactly 10.0 mL of this diluted solution and add it to a 250-mL volumetric flask. After Ailing the volumetric flask to the mark with distilled water (indicating the volume of the new solution is 250. mL), what is the concentration of the diluted Na2CO3 solution?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_forward95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated with hydrogen sulfide gas. For example, nickel(II) precipitates nearly quantitatively as NiS when H2S gas is bubbled through a nickel ion solution. How many milliliters of gaseous H2S at STP are needed to precipitate all (he nickel ion present in 10. mL of 0.050 M NiCl2 solution?arrow_forwardThree acid samples are prepared for titration by 0.01 M NaOH: 1 Sample 1 is prepared by dissolving 0.01 mol of HCl in 50 mL of water. 2 Sample 2 is prepared by dissolving 0.01 mol of HCl in 60 mL of water. 3 Sample 3 is prepared by dissolving 0.01 mol of HCl in 70 mL of water. a Without performing a formal calculation, compare the concentrations of the three acid samples (rank them from highest to lowest). b When the titration is performed, which sample, if any, will require the largest volume of the 0.01 M NaOH for neutralization?arrow_forward
- Chromium(III) chloride forms many compounds with ammonia. To find the formula of one of these compounds, you titrate the NH3 in the compound with standardized acid. Cr(NH3)xCl3(aq) + x HCl(aq) x NH4+(aq) + Cr3+(aq) + (x + 3) Cl(aq) Assume that 24.26 mL of 1.500 M HCl is used to titrate 1.580 g of Cr(NH3)xCl3. What is the value of x?arrow_forwardThe amount of oxygen, O2, dissolved in a water sample at 25 C can be determined by titration. The first step is to add solutions of MnSO4 and NaOH to the water to convert the dissolved oxygen to MnO2. A solution of H2SO4 and KI is then added to convert the MnO2 to Mn2+, and the iodide ion is converted to I2. The I2 is then titrated with standardized Na2S2O3. (a) Balance the equation for the reaction of Mn2+ ions with O2 in basic solution. (b) Balance the equation for the reaction of MnO2 with I in acid solution. (c) Balance the equation for the reaction of S2O32 with I2. (d) Calculate the amount of O2 in 25.0 mL of water if the titration requires 2.45 mL of 0.0112 M Na2S2O3 solution.arrow_forwardWhat volume of a 0.123 M hydrochloric acid solution is required to neutralize 13.3 mL of a 0.115 M barium hydroxide solution? _______ mL hydrochloric acidarrow_forward
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