The strength of a phosphoric acid sample is found to be 40% P2O5 by weight. Find the actual concentration of H3PO4 (weight %) in the acid.

Given the following information: hydrocyanic acid HCN nitrous acid Ka = 4.0×10-10 HNO₂ K₂ = 4.5×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.370 M aqueous hydrocyanic acid and sodium nitrite are mixed. It is not necessary to include states such as (aq) or (s). (2) At equilibrium the ( reactants OR products) will be favored. (choose one answer) (3) The pH of the resulting solution will be ( greater than, equal to, OR less than 7). (choose one answer)

D Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. Note: Solution 1 (Choose one) 2 = H₂O Explanation Solution 3 (Choose one) ▼ W S ▼ Check 3 747 E D (Choose one) Solution 2 $ (Choose one) 4 Solution 4 R % 5 T X 80 G 6 3 MacBook Pro Y & 7 H © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A U 8 J 1 ( 9 ➡ K ) O O P O

Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places. (a) (i) Write an expression for pH. (b) (ii) Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-³ hydrochloric acid are added to 990 cm³ of water. The acid dissociation constant, Ka, for the weak acid HX has the value 4.83 x 10-5 mol dm-³ at 25 °C. A solution of HX has a pH of 2.48 Calculate the concentration of HX in the solution. Page 4 of 14

< Interconverting pH and hydronium ion concentration 1:23 solution A B Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Be sure each entry you write ind correct number of significant digits. с H₂O*] PH 5.9 x 10-12 mol/L mol/L 6.1 x 10 mol/LO 1.22 Today 1:22 AM 317 .5G → Edit رت Ep

Titrations are acid-base reactions in which the amount of acid and base in solution are known quite precisely. The specific case where the acid and base have been added in equivalent molar amounts, is called the equivalence point. At this point, mol acid = mol base %3D At all other points in a titration, either the base is the limiting reactant (and there is excess acid) or the acid is the limiting reactant (and there is excess base). So, except at the equivalence point, titration problems are limiting reactant problems, which means we can do them- a lot of them! One additional point: when there is left over strong acid (acid in excess), 100% of that excess acid is ionized to become H* ions: [strong acid] = [H*] and pH = -log[H"] Something similar happens for strong bases. 1. Calculate the pH of the solution after the following amounts of 0.250 M NaOH have been added to 50.0 mL of 0.200 M HCI. Show all your work for each calculation (including the volumes for which the pH is given).…

The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is: Group of answer choices 2H+ (aq) + 2OH- (aq) → 2H2O (l) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)

A 0.050 M solution of the salt NaA has a pH of 9.00. Determine the [OH] and the pH of a 0.010 M solution of the acid HA. Show your work in the question parts below. Determine the equilibrium concentration of H3O* using the acid ionization equation. Recall that [OH] = 1.0 x 10-5. Consider the ionization equation described below.. HA(aq) + H20(1) =H;O*(aq) + A (aq) 1 Based on the given information, set up the ICE table in order to determine the unknown equilibrium concentration of all reactants and products. НА(ag) H20(1) H;O*(aq) А (ag) + Initial () Change () Equilibrium () 5 RESET 0.010 0.050 +x -2х +2x -x 0.010 + x 0.010 - x 0.050 + x 0.050 - x 0.010 + 2x 0.010 - 2x 0.050 + 2x 0.050 - 2x

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Bromothymol blue is yellow in acid solutions.  HBB is acidic form of the indicator . The indicator is blue in basic solutions.  BB- is  basic form of the indicator.             HBB    +     H2O         H3O+      +    BB-                      In this case, HBB is an acidic form of the indicator. BB- is the basic form of the indicator. The acidic form is yellow in color and the basic form is the blue color.    (a) Predict what will happen if NaOH is added to the reaction system.  explain why ?    make sure to explain why?