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Concept explainers
(a)
Interpretation: When magnesium of mass 0.121 g is dissolved in 50.0 mL of 1.00 M HCl, some amount of
Concept Introduction:Limiting reagentis the reactant that limits the amount of product produced in a
(b)
Interpretation: The volume of HCl in mL needs to be calculated at given temperature and pressure.
Concept Introduction:From theideal
Here, n is number of moles, R is Universal gas constant, T is temperature and P is pressure of the gas.
(c)
Interpretation: The joules of energy released by the magnesium needs to be determined.
Concept Introduction:Heat produced can be calculated as follows:
Where m is the mass, s is the specific heat capacity, delta T is the change in temperature.
The mass of the substance is related to number of moles and molar mass as follows:
(d)
Interpretation: The heat of reaction for magnesium needs to be calculated in joules/gram and in kilojoules/mol.
Concept Introduction:Heat released in J/g =
Heat released in kJ/mol =
1kJ = 1000J
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Chapter 16 Solutions
Pearson eText Basic Chemistry -- Instant Access (Pearson+)
- At 20°C, the solubility of potassium carbonate, K2CO3, is 110.3 g/100. mL of water. In the laboratory, a student mixes 215 g of K2CO3 with 175. g of H2O at a temperature of 20°C. (9.3) a) How much of the K2CO3 will dissolve? b) Is the solution saturated or unsaturated? c) What is the mass, in grams, of any solid K2CO3 left undissolved on the bottom of the container?arrow_forward9.118 A solution is prepared by dissolving 22.0 g of NaOH in 118.0 g of water. The NaOH solution has a density of 1.15 g/mL. (9.4) a. What is the mass percent (m/m) of the NaOH solution? b. What is the total volume, in milliliters, of the solution? c. What is the mass/volume percent (m/v) of the solution? d. What is the molarity (M) of the solution?arrow_forward(10.2) Calculate the fluoride ion concentration and pH of a solution that is 0.20 M in HF and 0.10 M in HCl. Ka 6.8 × 10¬4arrow_forward
- This is possible because of the following reactions that take place rapidly as long as reactants are available: (11.3) Equation : 51-(aq) + IO-3(aq) + 6H+(aq) ----> 3I2(aq) +3H2O(I)arrow_forwardBarium Hydroxide has a solubility of 4.68 g Ba(OH)2 in 100. g H2O at 25°C. Determine if each of the following solutions will be saturated or unsaturated at 25°C: (9.3) a) adding 32 g of Ba(OH)2 to 990 g of H2O b) adding 7.0 g of Ba(OH)2 to 125 g of H2O c) adding 22 g of Ba(OH)2 to 350. g of H2Oarrow_forward8) What is the pH of a solution containing 0.280 M weak base, B', with a K, of 3.9 X 107? (10.51) в (ад) + H-0 (1) ВН (аq) + ОН (ад)arrow_forward
- (14.6) Which of the following aqueous solution has the highest boiling point? O 1.00 M NaCl O 1.00 M Ca(NO3)2 O 1.00 M C6H1206 O 1.00 M NaNO3arrow_forward(5.7: Similar to For practice 5.11)The titration of a 20.0 mL sample of an H₂SO4 solution of unknown concentration requires 18.88 mL of a 0.203 M KOH to reach the equivalence point. What is the concentration (in M) of the unknown H₂SO4 solution? (Hint: Write the balanced reaction equation first.) O 0.0958 M O 0.383 M O 0.767 M O 0.192 Marrow_forwardH₂O₂ + KMnO4 + H₂SO4 O₂ + MnSO4 + K₂SO4+H₂O 1. How many moles of the oxidized product is formed in the reaction? (2,1,3,4) 2. How many electrons does the reducing agent loss?(5,3,7,1)arrow_forward
- What is the pH of a 0.25 M solution of a strong acid? (0.6)arrow_forward1. 8 mol of and 5 mol of nitrogen were in a 4L reaction vessel. When had been established with the product, ammonia gas, the concentration of the hydrogen gas was found to be 1 M. Find the equilibrium constant for the tio reaction. (0.48)arrow_forward5.14 What is the molar concentration of chloride ion in a solution prepared by dissolving 22.0 g of calcium chloride (FW= 111.1 g/mol) to 4.0L with water?arrow_forward
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