Is the pH of the solution at the equivalence point acidic, neutral, or basic for the following acid-base titration?

Formic acid (HCOOH) and KOH

The following titration curve was obtained when a 25.00 mL sample of HCl solution was titrated against 0.200 M NaOH solution. Calculate the morality of the HCl solution.

A 0.451-g sample of an unknown monoprotic acid is titrated with 0.150 M NaOH. The resulting titration curve is shown here. Determine the molar mass and pK_a of the acid.

The pH of a substance changes from 1 to 3. Determine the most suitable indicator to detect this pH change based on the figure below.

The following are representations of the initial concentrations of a weak acid HA (pKa = 6.15) and its potassium salt KA. Draw a representation of the equilibrium state of solution (4) upon the addition of 1 OH⁻ ion. (The potassium ions and water molecules were omitted for clarity).

A 1.0-L buffer solution is 0.125 M in HNO₂ and 0.145 M in NaNO₂. Determine the concentrations of HNO₂ and NaNO₂ after the addition of each substance: a. 1.5 g HCl

A 45.0 mL solution of 0.180 M CsOH solution is titrated with 0.100 M HI. Calculate the volume of the acid required to reach the equivalent point of the titration.

One of the following graphs represents the titration of a triprotic acid with a strong base. Which titration curve is it?

At 27 °C, a saturated solution of magnesium carbonate has an osmotic pressure of 98 torr. Calculate its solubility product constant at this temperature 

When KOH(aq) is added to the solution, will the solubility of Ni(OH)₂ increase, decrease, or remain the same? Give the balanced net ionic equation for the dissolution process. [Hint: Refer to complex ions formations]

If 75 mL of a solution made by dissolving 10.0 g of Ba(OH)₂(K_sp = 5.0×10^–3) in 300 mL of water was added to each of the beakers below, which beaker will a precipitate form? What is the identity of the precipitates that formed?

Based on the following qualitative analysis flowchart, how can you separate Bi³⁺ ion and Ba²⁺ ion contained in a solution?

What is the molar solubility of AgCN in 1.00 M NaCN solution? Use the following values: K_sp AgCN = 6.0×10^–17 and K_f [Ag(CN)₂]^– = 3.0×10²⁰.

Which of the following statements are correct? 

i. The reverse direction of a spontaneous reaction will be nonspontaneous under the same reaction conditions. 

ii. Spontaneous processes are slow. 

iii. All reversible reactions are spontaneous. 

iv. There is no heat loss in an isothermal process. 

v. A reversible process can produce more work than an irreversible process

Identify which among NH₃(g) and C₆H₆(g) have the higher standard molar entropy (S°) at 25 °C. Briefly explain.

When heated to 300 °C, sodium azide (NaN₃) decomposes to give elemental sodium and nitrogen gas.

2 NaN₃(s) → 2 Na(s) + 3 N₂(g)

Determine if the reaction is spontaneous at 1 atm and 25 °C.

The ∆H_vap and ∆S_vap for acetone are 31.3 kJ/mol and 95 J/(K·mol), respectively. What is the ΔS_surr and ΔS_total at 60 °C?

There are two possible ways to roll a 3 using two dice each numbered 1-6. Therefore, there are two microstates for the outcome of 3 (a specific microstate). Determine the number of possible ways to roll a 4. Calculate the entropy associated with an outcome of 4. (K_B = 1.38×10^–23)

Identify the sign of ΔS_sys and ΔS_surr for the reaction below without doing calculations and identify which temperature condition in which the reaction would be spontaneous

2 C₆H₆(l) + 15 O₂(g) → 12 CO₂(g) + 6 H₂O(l) ΔH°_rxn = -6534 kJ

Using the following data, 

P_N2 = P_PH3 = 0.06 atm, P_NH3= 0.3 atm, P_P4 = 0.2 atm

ΔG°_{f, P4(g)} = 24.4 kJ/mol, ΔG°_{f, NH3(g)} = –16.4, ΔG°_{f, PH3(g)} = 13.5 kJ/mol, ΔG°_{f, N2(g)} = 0

calculate K_p and ΔG at 298 K for the reaction 

4 PH₃ (g) + 2 N₂ (g) ⇌  P₄ (g) + 4 NH₃ (g)