Stoichiometry of Reactions Between Ions in Solutions

Key Questions

• How are stoichiometry and molarity related?

  Answer:

  Well, stoichiometry requires EQUIVALENCE with respect to mass and charge....

  Explanation:

  And for an older treatment of the principles involved, see [this old answer.](https://socratic.org/questions/can-you-explain-balancing-chemical-equations-in-detail) And the fundamental principle of stoichiometry is `"garbage in equals garbage out"`. Every chemical reaction must be balanced with respect to mass and charge. A `10*g` mass of reactants from all sources yields at most a `10*g` mass of products.

  `"Molarity"` is a concentration term, i.e. `"molarity"="moles of solute"/"volume of solution"`...and as such it has the units of `mol*L^-1`.. And so if we have TWO of the three quantities, say `"molarity"` and `"volume"`, we can get the third..`"moles of solute"`...

  …`"molarity"xx"volume"="moles"`....and this is certainly consistent dimensionally. What do I mean by this?

  And a practical example? Well suppose I gots a `100*mL` volume of `HCl(aq)`, that is `1*mol*L^-1` with respect to `HCl`. What mass of sodium hydroxide is required for equivalence?

  We write out the stoichiometric equation as a preliminary:

  `HCl(aq) + NaOH(aq)rarr NaCl(aq) +H_2O(l)`

  `n_"HCl"=0.100*Lxx1*mol*L^-1=0.100*mol`

  And for equivalence we require equimolar sodium hydroxide...

  `0.100*molxxunderbrace(40.0*g*mol^-1)_"molar mass of NaOH"=4.00*g`...i.e. a `4*g` mass of hydroxide is required for equivalence.

  anor277 · 1 · Jul 16 2018
• How can the knowledge of stoichiometry help us to resolve reactions between ions in solutions?

  Answer:

  How? The idea that not only mass is conserved but charge is conserved is a tenet of stoichiometry.

  Explanation:

  At its simplest level, stoichiometry embodies conservation of mass. If there are 10 g of reactant, at most there can be 10 g of product. But while mass is conserved in a chemical reaction; charge is also conserved. When we represent a redox reaction we use the addition/removal of electrons to represent reduction/oxidation respectively. Cross multiplication of the individual redox reactions shows how charge is conserved.

  anor277 · 1 · Nov 5 2015

• How do you measure concentration of reducing sugars?
• If 525 mL of 0.80 M HCl solution is neutralized with 315 mL of Sr(OH)2 solution what is the molarity of the Sr(OH)2? __ HCl + __ Sr(OH)2
  __ SrCl2 + __ H2O
• Why is stoichiometry called stoichiometry?
• How many grams of solid BaSO4 will form when Na2SO4 reacts with 25 mL of 0.50 M Ba(NO3)2? __ Ba(NO3)2 + __ Na2SO4
  __ BaSO4 + __ NaNO3
• How many liters of a 0.75 M solution of Ca(NO3)2 will be required to react with 148 g of Na2CO3? __ Ca(NO3)2 + __ Na2CO3
  __ CaCO3 + __ NaNO3
• If 45 mL of a 1.5 M AgNO3 is added to KCl how many grams of AgCl can be formed? __ AgNO3 + __ KCl
  __ AgCl + __ KNO3
• How many grams of sodium can react with 750 mL of a 6.0 M solution of sulfuric acid, H2SO4? __ Na + __ H2SO4
  __ Na2SO4 + __ H2
• How many grams of aluminum are required to react with 35 mL of 2.0 M hydrochloric acid, HCl? __ HCl + __ Al
  __ AlCl3 + __ H2
• How does gas stoichiometry differ from stoichiometry of solids and liquids?
• How does stoichiometry relate to the law of conservation?
• How are stoichiometry and molarity related?
• How can the knowledge of stoichiometry help us to resolve reactions between ions in solutions?
• How many grams of solid calcium hydroxide, Ca(OH)2, are required to react with 350 mL of 0.40 M HCl? __HCl + __Ca(OH)2
  __CaCl2 + __H2O
• How many moles are there in 6.37 x 10(-2) L of 0.0832 M barium nitrate?
• What are some common mistakes students make with stoichiometry of reactions between ions in solutions?
• What is an example of a stoichiometry of reactions between ions in solutions practice problem?
• What volume of 0.130 mol/L hydrochloric acid do you need to precipitate 1.64 g of lead(II) chloride from a solution of lead(II) nitrate?
• Question #1e60f
• Question #273c3
• Does a precipitate form when the aqueous solutions `"Ba(NO"_3)_2"` and `"2KOH"` are combined?
• Question #0e4b8
• Question #7e402
• Question #16531
• How many grams of copper are required to replace .5 moles of silver nitrate (which is dissolved in water), assuming a copper (II) product?
• What volume of 0.181 M `Na_3PO_4` solution is necessary to completely react with 91.0 mL of 0.107 M `CuCl_2`?
• Question #3b5f1
• Question #b716d
• A solution contains 1.77 g of dissolved silver. How many moles of potassium chloride must be added to the solution to completely precipitate all of the silver? What mass of potassium chloride must be added?
• Question #fe05d
• Question #05bc4
• Question #814fe
• What is `[HCl]` if a `17.04*mL` volume of `0.468*mol*L^-1` concentration of `[Ca(OH)_2]` was titrated with `13.7*mL` of said acid?
• Question #1dc6a
• Assume that 50 g of `KCl` is dissolved in 100 g of water at 100 °C and the solution is allowed to cool to 20°C. How much `KCl` remains in solution? How much `KCl` crystallizes from the solution?
• Question #c41c6
• How do ionic equations work?
• Am I doing this right? What mass of `"HCl"` reacts with `"3.26 g"` of `"Mg"("OH")_2`?
• Question #dead2
• What volume of 0.320 M `KOH` is needed to react completely with 23.4 mL of 0.220 M `H_2SO_4`?
• A 0.100 M solution of an acid, HA, has a pH = 2.00. what is the value of the ionization constant, `K_a` for this acid?
• Question #efffa
• `2xx10^-3*L` of `NaOH` of `0.200*mol*L^-1` concentration is added to `1.00*L` of `1.00*mol*L^-1` `Ca(NO_3)_2(aq)`...will calcium hydroxide precipitate?
• Given that for `Ca(OH)_2`, `K_"sp"=4.8xx10^-6`, will precipitation occur if a `125*mL` volume of calcium chloride at `2.9xx10^-2*mol*L^-1` concentration is mixed with a `175*mL` volume of sodium hydroxide at `2.9xx10^-2*mol*L^-1` concentration?
• What volume of a 1.0 M HCI is required to completely neutralize 25.0 ml of a 1.0 M KOH?
• Question #2cabc
• Question #6303e
• Question #9d048
• Will sodium fluoride and calcium nitrate react to produce a precipitate?
• How do we find gram solubilities of metal hydroxides?
• Solutions of `Li_2CO_3` and `MgCl_2` are mixed. a) What is the formula of the precipitate that forms? b) Write the equation for the reaction. c) Write the equation in ionic form. d) What is the net ionic equation of the reaction?
• What volume of `HCl(g)` is required for equivalence to a `32*mL` volume of `AgNO_3(aq)` at `0.08*mol*L^-1` concentration?
• How would you prepare 72.5 g of an aqueous solution that is 5.00% potassium iodide, KI, by mass?
• What mass of anhydrous salt is required to prepare a `50*g` mass of `"acetic acid trihydrate"`, `H_3C-CO_2H*3H_2O`?
• Given that `K_"sp"=4xx10^-13` for `"silver bromide"`, what will be the concentration of silver ion if `[Br^-]=1xx10^-6*mol*L^-1`?
• The concentration of Ag+ ions is 1x10^-6 M in AgBr solution. Find minimum concentration of Br- ions necessary to cause precipitation of AgBr. ( Ksp of AgBr= 4x10^-13 M^2)?
• What volume of 0.200 M K2C2O4 is required to completely react with 30.0 mL fo 0.100 M Fe(NO3)3?
• How do you calculate the moles and grams of solute in a solution of `5.0 x 10^2` mL of 2 M `KNO_3`?
• Question #a3ed1
• Will `"AgNO"_3` form a precipitate in an aqueous solution?
• What will occur when a `100*mL` volume of `AgNO_3(aq)` at `0.400*mol*L^-1` concentration is added to an excess of potassium chromate, `K_2^(+)[CrO_4]^(2-)`?
• Question #68eca
• What mass of `"lead chloride"` would result if a `21.5*mL` volume of `"lead nitrate"` at `0.0806*mol*L^-1` concentration were mixed with a `18.00*mL` volume of `"potassium chloride"` at `0.683*mol*L^-1` concentration?
• What volume of .150 M potassium iodide solution will completely react with .155 L of .112 M lead (II) nitrate? equation: 2KI (aq) + Pb(NO3)2 (aq) ----> 2KNO3 (aq) + PbI2 (s)
• If `"100 mL"` of `"0.01 mol/L"` tetraaquadichlorochromium(III) chloride reacts with excess silver nitrate, how many mols of silver chloride get produced?
• 25 mL of 0.350 M `"NaCl"` are added to 45 ml of 0.125 M `"CuSO"_4`. How many grams of `"Cu"("OH")_2` will precipitate?
• `(i)` What volume of `5.00*mol*L^-1` `HCl(aq)` is required to react with a `17.0*g` mass of sodium hydroxide. `(ii)` what volume of sodium sulfide at `0.100*mol*L^-1`, is required to precipitate a `33.0*mL` volume of `0.100*mol*L^-1` of `AgNO_3`?
• If excess of `AgNO_"3"` solution is added to 100 ml of 0.024 M solution of dichlorobis (ethylene diamine) cobalt (III) chloride, how many moles of `AgCl` will be precipitated??
• What is the mass of precipitate formed when 50 ml of 16.9% w/v solution of AgNO3 is mixed with 50 ml of 5.8% w/v NaCl solution?
• How many mL of a `"0.250 mol L"^(-1)` `"BaCl"_2` solution is required to precipitate all the sulfate ions from `"10.0 mL"` of a `"10.0 % (w/v)"` solution of `"Na"_2"SO"_4` ?
• Question #d6e76