What is the information needed to know if Ksp will increase or decrease with temperature? What is the effect on Ksp when temperature is increased?

Which of the following insoluble salts will have a greater solubility at a lower pH. 1. BaC204 2. SRSO4 3. Fe(OH)3 o None of them o 1 only O 2 only O 3 only o 1 and 2 o 1 and 3 O 2 and 3 O All of them

Write the net ionic equation for the precipitation reaction that occurs when aqueous solutions of silver nitrate ( AGNO3(aq)) and potassium phosphate (K3PO4(aq)) are mixed. (a) Write a complete ionic equation and (b) a net ionic equation. (c) Which ones are spectator ions? Use the editor to format your answer

18.57grams of Ce(NO3)4 are required to make the solution. (I don't know if you need that information to solve this question but that is the answer to question a)

If NH4OH at 30.0 °C is 1.20 % ionized is 0.250 M solution, what is its ionization constant and the % ionization in 0.500 M solution?                                              NH4OH    ↔       NH4+      +        OH- I 0.250 0 0 C 0.012(0.250) 0.012(0.250) 0.012(0.250) E       Kb =  I 0.500 0 0 C -x +x +x E       % I= x / 0.5 x 100

Which of the following buffer would work best for making a buffer at pH 7.5? O TAPS, K₂ = 4.0 x10⁹ O HEPES, K₂= 3.2 x10-8 O Acetic acid, K₂ = 1.6x10-5 O CAPS, K₂ = 4.0 x10-¹¹ O PIPES, K₂ = 1.6 x10-7

Predict whether the following will fully dissociate, partially dissociate, or not dissociate when dissolved solution. Provide a balanced equation for the hyderation of each compound. 1) NaI (s) Sodium iodide. 2) Pyruvic ACID HO 3) glucose H₁2 (s)

30. Indicate the FALSE statement about pH indicators and their use in titrations: A) A pH indicator suitable for titrations of strong bases with strong acids cannot be used for titrations of strong acids with strong bases. B) pH indicators should be used sparingly (in small amounts) as they are weak acids/ bases, and thus could affect the volume of titrant used. C) An indicator should be selected such that its pKits value matches the equivalence point pH. D) pH indicators all contain at least one acidic group that can be deprotonated to form a differently colored conjugate base. E) The colours of the acid and base forms of a given pH indicator depend on their chemical structures.

Write a few sentences that describe the relationship between CO2 and pH of the blood.

For each of the following pairs of substances, predict which member of the pair will have the higher IMF, and indicate why. NaF and MgO   Na2O and SiC   HCl and HF   Ar and NO