Strong Acid VS Weak Acid Reaction Rate

[polkadot]

I know that the equilibrium constant does not indicate rate of reaction, but suppose you have two solutions with the same concentration and volume, one with HCL and one with ethanoic acid, and you add the same mass of calcium carbonate to each one. Would it be correct to conclude that because HCL ionises to a greater extent than ethanoic acid, it has a greater concentration of ions, therefore more successful collisions, therefore greater reaction rate?
Or not?

Thanks

[Mao]

I know that the equilibrium constant does not indicate rate of reaction, but suppose you have two solutions with the same concentration and volume, one with HCL and one with ethanoic acid, and you add the same mass of calcium carbonate to each one. Would it be correct to conclude that because HCL ionises to a greater extent than ethanoic acid, it has a greater concentration of ions, therefore more successful collisions, therefore greater reaction rate?
Or not?

Thanks

Even though HCl does react faster than CH3COOH, the logic is flawed.

More collisions does not mean faster reaction rate. The activation energy of two reactions can be very different, and it's not easy to compare two reactions to each other.

[Nobby]

I know that the equilibrium constant does not indicate rate of reaction, but suppose you have two solutions with the same concentration and volume, one with HCL and one with ethanoic acid, and you add the same mass of calcium carbonate to each one. Would it be correct to conclude that because HCL ionises to a greater extent than ethanoic acid, it has a greater concentration of ions, therefore more successful collisions, therefore greater reaction rate?
Or not?

Thanks

Even though HCl does react faster than CH3COOH, the logic is flawed.

More collisions does not mean faster reaction rate. The activation energy of two reactions can be very different, and it's not easy to compare two reactions to each other.

Aren't both reactions essentially going to have H⁺ as a reactant though, as opposed to HA?

[polkadot]

Oh okay, thank you!

I know that the equilibrium constant does not indicate rate of reaction, but suppose you have two solutions with the same concentration and volume, one with HCL and one with ethanoic acid, and you add the same mass of calcium carbonate to each one. Would it be correct to conclude that because HCL ionises to a greater extent than ethanoic acid, it has a greater concentration of ions, therefore more successful collisions, therefore greater reaction rate?
Or not?

Thanks

Even though HCl does react faster than CH3COOH, the logic is flawed.

More collisions does not mean faster reaction rate. The activation energy of two reactions can be very different, and it's not easy to compare two reactions to each other.

Aren't both reactions essentially going to have H⁺ as a reactant though, as opposed to HA?

What I was thinking was that HCL would have more H+ than ethanoic acid, but I guess rate of reaction is influenced by many other factors..

[Mao]

Aren't both reactions essentially going to have H⁺ as a reactant though, as opposed to HA?

What I was thinking was that HCL would have more H+ than ethanoic acid, but I guess rate of reaction is influenced by many other factors..

My apologies. You (both) are correct. I didn't read the question properly.

In my defence, I had quite a few drinks that night. Don't drink and do chemistry.