How is the concentration of hydroxide ions

The concentration of an acid solution can be determined by titration with a strong base. First, calculate the number of moles of strong base required to reach the equivalence point of the titration. Then, using the mole ratio from the balanced neutralization equation, convert from moles of strong base to moles of acid. Finally, divide the number of moles of acid by the given volume of the acid solution to find the concentration. Created by Jay. When you divide both sides by 20 mL, the units cancel out so it does not matter what you choose. All that matters is that the unit you choose is the same throughout the equation. Dividing 27.4mL by 20mL is the same as dividing 0.0274L by 0.02L. You will get the same number and there will be no units! So, we can say that mL were used simply because the information was given in mL and it would have been unecessary to change. You have a base reacting with an acid. The question asks how much acid you need to react with base so that they neutralize each other (and form a salt with water, but no floating acids or bases). So, when are MV(basic)=MV(acidic). The greater volume that is made will not influence the equilibrium point because water is at pH 7 (neutral) so the ratio to total volume is irrelevant. Acids (using the Arrhenius definition) are chemicals which produce H+ ions, while bases are chemicals which produce OH- ions. So when barium hydroxide (Ba(OH)2) and hydrochloric acid (HCl) enter a water solution they will dissociate, or s...

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Jacob, pH is a measure of the amount of Hydrogen ions (H+) in a solution. Ions are just atoms that have an electric charge on them, so H+ is a hydrogen atom with charge of 1. Even in pure water ions tend to form due to random processes (producing some H+ and OH- ions). The amount of H+ that is made in pure water is about equal to a pH of 7. That's why 7 is neutral. For those who want a more complicated answer, pH is defined: pH = -log 10[H+], where [H+] is the concentration of H+ , expressed in moles/liter. In pure water near room temperature, the concentration of H+ is about 10 -7 moles/liter, which gives a pH of 7. I hope this answers your question. math dan (w. mike w) (published on 10/22/2007) The pH scale actually is based on another scale. We usually keep track of the concentration of solutes in moles per liter (M). The pH is minus the log (base 10) of the H + concentration in moles per liter. Since at room temperature in pure water, that concentration is very close to 10 -7 M, pH 7 is neutral. Mike W. (published on 09/17/2009) That's true. We implied that by describing the liquid as pure water, so that the formation of an H + always goes along with the formation of an OH -. In solutions with other ions (say Na + or Cl -) there's no such constraint, so the H + and OH - concentrations no longer equal. Thus NaOH forms a base, with lots of OH -, and HCl forms an acid, with lots of H +. Mike W. (published on 05/25/2012) OK, I think I follow all the answers so far... star...

Learning Objectives • To understand the autoionization reaction of liquid water. • To know the relationship among pH, pOH, and \(pK_w\). Because of its highly polar structure, liquid water can act as either an acid (by donating a proton to a base) or a base (by using a lone pair of electrons to accept a proton). For example, when a strong acid such as HCl dissolves in water, it dissociates into chloride ions (\(Cl^−\)) and protons (\(H^+\)). The proton, in turn, reacts with a water molecule to form the hydronium ion (\(H_3O^+\)): \[\underset\) is an equilibrium reaction as indicated by the double arrow and hence has an equilibrium constant associated with it. The Ion-Product Constant of Pure Water Because water is amphiprotic, one water molecule can react with another to form an \(OH^−\) ion and an \(H_3O^+\) ion in an autoionization process: \[\ce\] where \(a\) is the activity of a species. Because water is the solvent, and the solution is assumed to be dilute, the activity of the water is approximated by the activity of pure liquid water, which is defined as having a value of 1. The activity of each solute is approximated by the molarity of the solute. Note It is a common error to claim that the molar concentration of the solvent is in some way involved in the equilibrium law. This error is a result of a misunderstanding of solution thermodynamics. For example, it is often claimed that K a= K eq[H 2O] for aqueous solutions. This equation is incorrect because it is an err...

The So, if you have a compound that dissociates into cations and anions, the minimum concentration of each of those two products will be equal to the concentration of the original compound. Here's how that works: #NaCl_((aq)) -> Na_((aq))^(+) + Cl_((aq))^(-)# Sodium chloride dissociates into #Na^(+)# cations and #Cl^(-)# anions when dissolved in water. Notice that 1 mole of #NaCl# will produce 1 mole of #Na^(+)# and 1 mole of #Cl^(-)#. This means that if you have a #NaCl# solution with a concentration of #"1.0 M"#, the concentration of the #Na^(+)# ion will be #"1.0 M"# and the concentration of the #Cl^(-)# ion will be #"1.0 M"# as well. Let's take another example. Assume you have a #"1.0 M"# #Na_2SO_4# solution #Na_2SO_(4(aq)) -> 2Na_((aq))^(+) + SO_(4(aq))^(2-)# Notice that #Na_2SO_4# and #Na^(+)# is #1:2#, which means that 1 mole of the former will produce 2 moles of the latter in solution. This means that the concentration of the #Na^(+)# ions will be #"1.0 M" * ("2 moles Na"^(+))/("1 mole Na"_2"SO"_4) = "2.0 M"# Think of it like this: the volume of the solution remains constant, but the number of moles doubles; automatically, this implies that the concentration will be two times bigger for that respective ion. Here's how that would look mathematically: #C_("compound") = n_("Compound")/V => V = n_("compound")/C_("compound")# #C_("ion") = n_("ion")/V = n_("ion") * 1/V = n_("ion") * C_("compound")/n_("compound")# #C_("ion") = C_("compound") * n_("ion")/n_("compound")# As...

As discussed earlier, hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water ( K w). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is neutral if it contains equal concentrations of hydronium and hydroxide ions; acidic if it contains a greater concentration of hydronium ions than hydroxide ions; and basic if it contains a lesser concentration of hydronium ions than hydroxide ions. A common means of expressing quantities, the values of which may span many orders of magnitude, is to use a logarithmic scale. One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where “X” is the quantity of interest and “log” is the base-10 logarithm: \[\mathrm\; M\) (corresponding to pH values greater than 7.00 and pOH values less than 7.00). When pH=7 Solutions are not Neutral Since the autoionization constant \(K_w\) is temperature dependent, these correlations between pH values and the acidic/neutral/basic adjectives will be different at temperatures other than 25 °C. For example, the hydronium molarity of pure water at 80 °C is 4.9 × 10 −7 M, which corresponds to pH and ...