The balanced equation for the reaction of L i O H and B a ( O H ) 2 has to be written. Concept introduction: Balanced reaction is a chemical reaction in which number of atoms for each element in the reaction and the total charge are same on both reactant side and the product side. Steps in balancing the information Step 1: Write the unbalanced equation Step 2: Find the coefficient to balance the equation. The coefficient should be reduced to the smallest whole number
The balanced equation for the reaction of L i O H and B a ( O H ) 2 has to be written. Concept introduction: Balanced reaction is a chemical reaction in which number of atoms for each element in the reaction and the total charge are same on both reactant side and the product side. Steps in balancing the information Step 1: Write the unbalanced equation Step 2: Find the coefficient to balance the equation. The coefficient should be reduced to the smallest whole number
Solution Summary: The author explains that the balanced equation for the reaction of LiOH and Ba(OH)_2 has to be written.
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
Chapter 4, Problem 4.119QP
(a)
Interpretation Introduction
Interpretation:
The balanced equation for the reaction of LiOH and Ba(OH)2 has to be written.
Concept introduction:
Balanced reaction is a chemical reaction in which number of atoms for each element in the reaction and the total charge are same on both reactant side and the product side.
Steps in balancing the information
Step 1: Write the unbalanced equation
Step 2: Find the coefficient to balance the equation.
The coefficient should be reduced to the smallest whole number
(b)
Interpretation Introduction
Interpretation:
Mass of CO2 that can be removed by given LiOH and Ba(OH)2 has to be calculated.
Concept introduction:
Mole:
The mole of the solute is calculated by multiplication of concentration of solution and volume of the solution and it is,
Mole=Concentration(M)×volume(L)
Molarity = No. of moles of soluteVolume of solution in L
Mass:
The mass of solute present in the solution is given by multiplication of mole and molar mass of the solute.
Mass=Mole×Molarmass
Molarmass=MassMole of solute
(c)
Interpretation Introduction
Interpretation:
Solution that is used in a space capsule and in submarine has to be identified.
Concept introduction:
Mass:
The mass of solute present in the solution is given by multiplication of mole and molar mass of the solute.
A solution is prepared by dissolving 2.95 g Co2(SO4)3 in enough water to make 1.00 L of red solution; the red color is due to the presence of the cobalt ions. To this solution was added 1.52 g of magnesium powder. A redox reaction occurred, in which the magnesium atoms lose all of their valence electrons and the red color of the solution fades.
(a) Write the total reaction that occurs and the net ionic equation for the redox process. (Assume that one of the products of the redox reaction is a metal.)
(b) Calculate the initial concentration of cobalt ions, the final concentration of cobalt ions, and the final concentration of magnesium ions.
Consider an analyte solution of 50.0 mL of 0.050 M hydrochloric acid, HCl, titrated against 0.10 M sodium hydroxide, NaOH.
(a) What is the chemical equation representing the titration reaction?
(b) At the start of the titration, before any NaOH is added, what ions or molecules are present in the solution? You only need to list chemical species that are present in appreciable quantities - anything that is considered a small enough concentration to where you’d make a small-change approximation on an ICE table doesn’t need to be included.
(c) Which of species you identified in part (b) will determine the pH of the solution?
A piece of chalk (mainly calcium carbonate) is placed in 250. mL of 0.337 M HCl.
All the CaCO3 reacts, releasing carbon dioxide gas and leaving 250. mL of a clear solution.
20.00 mL of the solution is pipetted into another flask.
37.6 mL of 0.0517 M NaOH is required to titrate the HCl remaining in this 20.00-mL portion.
What was the original mass of CaCO3 in the piece of chalk?
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell